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244 Cards in this Set
- Front
- Back
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noble gases |
They don’t combine with many other elements—chemically aloof, far right of periodic table, group 18/VIII
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neutrons
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neutral particles, n, add to mass
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nucleons
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neutrons and protons are grouped together as this
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atom
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smallest particle of an element
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atomic hypothesis
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1. all atoms of given element identical
2. atoms of different elements have different masses 3. compound is a specific comb of atoms of more than one element 4. in chem reaction, atoms are neither created nor destroyed; they exchange partners to produce new substances |
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element
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substance composed of only one kind of atom
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nuclear model
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an atom consists of a small positively charged nucleus, responsible for almost all of its mass, surrounded by negatively charged electrons
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electrons
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negatively charged particles surrounding nucleus to make up nuclear model of an atom; having a single negative charge per each
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protons
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positively charged particles inside the nucleus having a single positive charge per each
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atomic number
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number of protons in an element's atomic nucleus; denoted "Z"; for ex hydrogen has Z=1
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mass spectrometer
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device for determining the mass of an atom
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mass number
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total number of protons and neutrons in a nucleus, denoted "A"
which is also the atomic weight right? |
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isotopes
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atoms with the same atomic number but with different mass numbers, differences is in the number of neutrons
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neutron
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electrically neutral particles of an atom denoted "n"
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periodic table
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arrangement of elements that shows their family relationships
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groups
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vertical columns of the periodic table
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main groups or main group elements
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taller columns (Groups 1,2,&13/III through 18/VIII); could also be described as s-block and p-block
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periods
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horizontal rows
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blocks
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four rectangular regions of the period table; for reasons related to atomic structure are labeled "s" "p" "d" and "f"
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transition metals
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members of the "d" block. they transition from vigorously reactive metals in the "s" block and the less reactive metals on the left of the "p" block
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inner transition metals
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members of the f block which is shown below the main table to save space; parts of periods 6 and 7
Lanthanides period Actinides period |
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lanthanoids
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upper row of the inner transition metals beginning with lanthanum (it's in period 6)
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actinoids
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lower row of the inner transition metals beginning with actinium (it's in period 7)
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alkali metals
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elements in group 1, soft, lustrous metals that melt at low temperatures. they all produce hydrogen when they come in contact with water
Top to bottom: Li Na K Rb Cs Fr |
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alkaline earth metals
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elements in group 2, similar reactions as in group 1 except that their reactions are less vigorous
Be Mg Ca Sr Ba Ra |
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noble gases
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elements on the far right of the table in group 18/VIII, they combine with very few elements--chemically aloof; colorless, odorless gases
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halogens
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elements of group 17/VII, many of the properties of halogens vary in a regular fashion from F through Cl and Br to I, going from pale gas to colored gas to colored liquid to colored solid; All the halogens exist as diatomic molecules: F2, Cl2, Br2, I2
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metal
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conducts electricity, has a luster, is malleable and ductile
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nonmetal
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doesn't conduct electricity, neither malleable nor ductile
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metalloid
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has the appearance and some properties of a metal but behaves chemically like a nonmetal
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compound
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electrically neutral substance that consists of two or more different elements with their atoms present in a definite ratio
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binary compound
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consists of only two elements
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organic compounds
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contain the element carbon and usually hydrogen, too
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inorganic compounds
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all the other compounds that don't include carbon
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molecule
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a discrete group of atoms bonded together in a specific arrangement
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ion
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positively or negatively charged atom or molecule
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cation
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positively charged ion
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anion
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negatively charged ion
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ionic compound
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ions in a ratio that results in overall electrical neutrality
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molecular compound
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electrically neutral molecules
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chemical formula
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represents a compounds composition in terms of chemical symbols
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molecular formula
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chemical formula that shows how many atoms of each type of element are present in a single molecule of the compound
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diatomic molecules
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molecules that consist of two atoms; for instance molecules of hydrogen gas contain hydrogen atoms bonded together in a 2 of H2
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structural formula
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indicates how the atoms are linked together, but not their actual three-dimensional arrangement in space
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line structure
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represents a chain of carbon atoms by a zigzag line, where each short line indicates a bond and the end of each line represents a carbon atom
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space-filling model
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the atoms are represented by colored spheres that fit into one another
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ball-and-stick model
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each ball represents the location of an atom, and the sticks represent the bonds
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tube structure
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like ball and stick but without balls
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density isosurface
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gives a more accurate view of what it would look like but makes it hard to see where the atoms are
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electrostatic potential surface
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"elpot" surface in which the net electric potential is calculated at each point of the density isosurface and depicted by different colors
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monatomic ions
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single-atom ions
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diatomic
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ions that consist of two atoms bonded together (example is cyanide ion which is CN-)
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polyatomic
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three or more atoms bonded together (example is ammonium ion NH4+)
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oxoanions definition
+ 5 basic formula templates |
most common polyatomic anions, polyatomic anions that contain oxygen...they include the
nitrate NO3- chlorate ClO3- carbonate CO3 2- sulfate, SO4 2- phosphate PO4 3- |
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binary ionic compound
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a compound formed from ions of two elements (for example CaCl2, formed from Ca2+ and Cl- in the ratio of 1:2
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common names
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informal names like "water" or "salt" that were known before the chemical composition
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systematic name
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reveals which elements are present and in some cases the arrangement of atoms
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chemical nomenclature
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systemic naming of compounds
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oxidation number
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when an element can form more than one kind of cation, such as Cu+ and Cu2+, the charge of the cation, written as a Roman numeral in parentheses following the name of the element. Cu+ = copper(I) ion and Cu2+ = copper (II) ion
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hydrates
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ionic compounds that form crystals that incorporate a definite proportion of molecules of water as well as the ions of the compounds itself; an example copper(II) sulfate normally exists as blue crystals of compositions CuSO4*5H2O
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anhydrous
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when we wish to emphasize that the compound has lost its water of hydration; thus CuSO4 is anhydrous copper(II) sulfate
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hydrocarbons
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compounds of hydrogen and carbon; they include methane, CH4, ethane, C2H6, and benzene, C6H6
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alkanes
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hydrocarbons that have no carbon-carbon multiple bonds
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alkenes
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hydrocarbons with double bonds; ethene, CH2=CH2, is the simplest example of an alkene
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aromatic compounds
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hydrocarbon with double bonds with distinct properties like the exceptionally stable hexagonal benzene ring
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alcohol
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a type of organic compound that contains an -OH group
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carboxylic acid
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a compound that contains the carboxyl group - COOH
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haloalkane
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an alkane in which one or more H atoms have been replaced by halogen atoms
example: chloromethane, CH3Cl example: trichloromethane, CHCl3 |
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mole
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1 mole of objects contains the same number of objects as there are atoms in exactly 12 g of carbon-12 (abbreviated mol)
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amount of substance
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denoted italic n
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Avogadro's constant
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number of objects per mole, 6.0221 x 10to23 mol-1
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atomic weight
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the numerical value of its molar mass
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molecular weight
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the molecular weight of a molecular compound is the numerical value of its molar mass
goes with molecular compound where ionic compounds are called formula weight and not molecular weight |
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formula weight
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formula weight of an ionic compound is the numerical value of its molar mass
goes with ionic compound where molecular weight goes with a molecular compound |
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empirical formula
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shows the relative numbers of atoms of each element present in the compound. Empirical formula is the lowest common denominator showing ratios... for example, C2H4O2 and C3H6O3 both have the same empirical formula of CH2O
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homogeneous mixture
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the molecules or ions of the components are so well mixed that the composition is the same though, no matter how small the sample
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solution
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a homogeneous mixture is also called a solution
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solvent
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usually the component of the solution present in the larger amount is called the solvent
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solute
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any dissolved substance
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crystallization
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takes place when the solute slowly comes out of solution as crystals, perhaps as the solvent evaporates
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precipitation
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a solute comes out of solution so rapidly that a single crystal does not have time to form. Instead, the solute forms a finely divided powder called a precipitate. This is almost always instantaneous
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aqueous solutions
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solutions in which the solvent is water
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nonaqueous solutions
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solutions in which the solvent is not water
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solid solutions
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the solvent is a solid; an example is a common form of brass that can be regarded as a solution of copper in zinc
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filtration
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used to separate substances when there is a difference in solubility
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decanting
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makes use of differences in density. One liquid floats on another liquid or lies above a solid and is poured off
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chromatography
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one of the most sensitive techniques available for separating a mixture. relies on the different abilities of substances to adsorb, or stick to surfaces. discussed in detail later
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adsorb
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stick to surfaces
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distillation
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makes use of differences in boiling points to separate mixtures
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stock dilution
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common space-saving practice in chemistry of storing a solution in a concentrated form
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dilute
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reduce its concetrated form
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volumetric flask
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a flask calibrated to contain a specified volume
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chemical reactions
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processes by which one or more substances are converted into other substances (same as chemical change)
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chemical change
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the type or process that causes one or more substance to be converted into other substances (same as chemical reactions)
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reactants
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the starting materials in chemical reactions
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products
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the substances formed from chemical reactions
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reagents
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the chemicals available in a laboratory used to make chemical reactions
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skeletal equation
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expresion that shows the bare bones of the reaction including the identities of the reactants and the products in terms of chemical formulas. a skeletal equation is a qualitative summary of a chemical reaction
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law of conservation of mass
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the observation that the total mass is constant during a chemical reaction; it just changes places
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balanced
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when a formula depicts atoms of different number and then multiply formulas by factors and end up with the same numbers of atoms on both sides of an aarow
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stoichiometric coefficient
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the number multiplying an entire chemical formula in a chemical equation... for example the 2 here: 2 Na + 2 H2O -> 2 NaOH + H2
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state symbol
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a chemical equation typically also shows the physical state of each reactant and product by using a symbol like (s) solid (l) liquid (g) gas (aq) aqueous solution
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catalyst
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a substance that increases the rate of a reaction but is not itself consumed in the reaction
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mass of electron
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e- has -1 charge and mass in kg of: 9.109 x 10to-31
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mass of proton
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p has +1 charge and mass in kg of: 1.673x10to-27
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neutron
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n has 0 charge and mass in kg of: 1.675 x 10to-27
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deuterium
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(D) superscript2H
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tritium
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(T) superscript3H
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carbonate's formula
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CO3 2-
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nitrates's formula
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NO3 -
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phosphate's formula
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PO4 3-
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sulfate's formula
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SO4 2-
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formula unit
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group of ions that make up an ionic compound. we don't say a "molecule" of an ionic compound, instead we say "formula unit"
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in old school chemistry, adding "-ous" to a cation (such as "ferrous" ions) would indicate what?
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lower charges. so ferrous ions would be iron(II)
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in old school chemistry, adding "-ic" to a cation (such as "ferric" ions) would indicate what?
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higher charges. so ferric ions would be iron(III)
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monatomic anions get what suffix in their name? An example is what?
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"-ide"
S2- is sulfide |
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the ions formed by the halogens are collectively called what?
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halide ions;
they include flouride (F-) chloride (Cl-), bromide (Br-), iodide (I-) |
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oxoanion
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ion that contains oxygen
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If only one oxoanion of an element exists, its name is formed by adding what suffix to the stem of the name of the element?
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"-ate"
an example is the carbonate ion, CO3superscript2- |
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If an element can form two types of oxoanions, with different numbers of oxygen atoms, which ending does the larger number of oxygen atoms get, and which ending does the smaller number of oxygen atoms get?
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"-ate" for larger number of oxygen atoms
"-ite" for smaller number of oxygen atoms E.g. NO3- = nitrate and NO2- = nitrite |
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F-
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flouride ion
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Cl-
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chloride ion
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Br-
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bromide ion
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I-
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iodide ion
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O2-
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oxide ion
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OH-
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hydroxide ion
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S2-
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sulfide ion
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HS-
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hydrogen sulfide ion
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CN-
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cyanide ion
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CH3COsubscript2upper-
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acetate ion
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COsubscript3upper2-
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carbonate ion
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HCOsubscript3upper-
and it's nickname is what? |
hydrogen carbonate ion
also called bicarbonate |
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NOsubscript2upper-
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nitrite ion
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NOsubscript3upper-
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nitrate ion
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POsubscript4upper3-
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phosphate ion
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HPOsub4super2-
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hydrogen phosphate ion / biphosphate
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Hsub2POsub4upper-
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dihydrogen phosphate ion
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SOsub3super2-
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sulfite ion
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HSOsub3upper-
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hydrogen sulfite ion
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SOsub4upper2-
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sulfate ion
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HSO4-
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hydrogen sulfate ion
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ClOsub2upper-
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chlorite ion
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ClOsub3upper-
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chlorate ion
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ClOsub4upper-
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perchlorate ion
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some elements--particularly halogens--form more than two kinds of oxoanions. The name of the oxoanion with the smallest number of oxygen atoms is formed by getting what prefix and suffix?
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prefix - "hypo"
suffix - "ite" |
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The oxoanion with the most oxygen atoms is named with what prefix?
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prefix - "per" such as perchlorate ion, ClOsub4upper-
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Lithium's typical ion
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Li+
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Beryllium's typical ion
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Be2+
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Sodium's typical ion
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Na+
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Aluminum's typical ion
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Al3+
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Magnesium's typical ion
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Mg2+
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Potassium's typical ion
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K+
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Calcium's typical ion
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Ca2+
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Gallium's typical ion
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Ga3+
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Rubidium's typical ion
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Rb+
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Cadmium's typical ion
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Cd2+
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Barium's typical ion
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Ba2+
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Copper's typical ion
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Cu+
Cu2+ |
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Radium's typical ion
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Ra2+
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Indium's typical ion
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In+
In3+ |
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Strontium's typical ion
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Sr2+
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Silver's typical ion
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Ag+
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Cesium's typical ion
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Cs+
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Zinc's typical ion
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Zn2+
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iron's typical ion
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Fe2+
Fe3+ |
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gold's typical ion
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Au+
Au3+ |
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mercury's typical ion
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Hgsub2super2+
Hg2+ |
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Thallium's typical ion
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Tl+
Tl3+ |
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lead's typical ion
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Pb2+
Pb4+ |
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tin's typical ion
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Sn2+
Sn4+ |
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nitrogen's typical ion
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N3-
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Oxygen's typical ion
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O2-
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Phosphorous's typical ion
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P3-
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Iodine's typical ion
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I-
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bromine's typical ion
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Br-
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Selenium's typical ion
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Se2-
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fluorine's typical ion
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F-
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Sulfur's typical ion
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S2-
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chlorine's typical ion
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Cl-
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oxoacid
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an acidic molecular compound that contains oxygen
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generally -ic oxoacids are the parents of oxoanions ending in what?
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-ate
for example: H2SO4 sulfuric acid becomes a sulfate ion if you remove the 2 hydrogen |
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generally -ous oxoacids are the parents of oxoanions ending in what?
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-ite
for example, H2SO3 sulfurous acid becomes the sulfite ion SOsub4super2- |
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in what way are oxoacids the parents of oxoanions?
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in the sense that an oxoanion is formed by removing one or more hydrogen ions from an oxoacid molecule
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carbon's typical ion
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either C 4+ or C 4- depending on the situation
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carboxyl group
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COOH
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haloalkanes have names beginning in which prefixes?
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fluro-
chloro- bromo- iodo- |
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common name for HCl(aq)
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hydrochloric acid
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common name for H2SO4(aq)
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sulfuric acid
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common name for HNO3(aq)
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nitric acid
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common name for CH3COOH(aq)
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acetic acid
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common name for H2SO3(aq)
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sulfurous acid
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common name for H3PO4(aq)
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phosphoric acid
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silicon's typical ion
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Si4+ usually or Si4- depending on conditions
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1 Mol equals what?
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6.0221 x 10to23 atoms in 12 grams of carbon-12
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formula for finding amount in mol
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N = n*NsubA
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NsubA
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Avogadro's constant
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molar mass
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M, of an element is the mass per mole of its atoms
M, of a molecular compound is the mass per mole of its molecules M, of an ionic compound is the mass per mole of its formula units |
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molar concentration
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c, (also called the "molarity" of the solute
equal to the amount of solute in moles divided by the volume of the solution in liters |
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what are the units of molarity?
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moles per liter
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soluble substance
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one that dissolves to a significant extent in a specified solvent
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insoluble substance
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doesn't dissolve significantly in a specified solvent
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electrolyte
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substance that, in a solution, is present as ions; ionic solutions that are soluble in water are electrolytes because the ions become free to move when the solid dissolves
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strong electrolyte
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substance that is present almost entirely as ions in solution; three types:
1. strong acids 2. strong bases 3. soluble ionic compounds |
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weak electrolyte
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substance that is incompletely ionized in solution; in other words, most of the molecules remain intact; acetic acid is a weak electrolyte
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how can you distinguish by measuring whether strong or weak electrolytes?
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ability of solutions to conduct electricity, strong is better
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acid
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compound that contains hydrogen and reacts with water to form hydrogen ions (H+)
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base
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produces hydroxide ions (OH-) in water
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Bronsted-Lowry definition of acids/bases
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acid = proton donor
base= proton acceptor |
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monoprotic acid
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an acid that can donate only one proton from each molecule
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polyprotic acid
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an acid that can donate more than one proton from each molecule; H2SO4 can release both its hydrogen atoms as ions
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strong acid
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completely deprotonated in solution
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weak acid
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incompletely deprotonated in solution
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strong base
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completely protonated in solution
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weak base
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incompletely protonated in solution
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reduction
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an atom gains electrons from another species
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reaction stoichiometry
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the quantitative aspect of chemical reactions; the key is the balanced chemical equation
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acid-base tritations
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an acid reacts with a base
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redox tritations
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reaction between a reducing agent and an oxidizing agent
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analyte
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the solution being analyzed
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tritant
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the solution containing a known concentration of reactant measured into the flask from a buret
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competing reaction
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reaction taking place at the same time as the one in which we are interested and using some of the same reactants
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theoretical yield
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maximum quantity (amount, mass, or volume) of product that can be obtained from a given quantity of reactant
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percentage yield
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fraction of the theoretical yield actually produced, expressed as a percentage
= actualyield/theoriticalyield x100% |
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limiting reactant
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reactant that governs the maximum yield of the product
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force
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F, an influence that changes the state of motion of an object. This means it can change an objects magnitude or direction or both
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acceleration
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a, of the object is the rate of change of its velocity and is proportional to the force that it experiences
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velocity
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rate of change of position; has both magnitude and direction
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speed
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v, magnitude of the velocity of an object, regardless of the direction of the motion
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energy
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capacity to do work
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joule
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SI unit for energy
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1 J =
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1 J = 1 kg*m2*s-2
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kinetic energy
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EsubK, the energy that a body possesses due to its motion. body of mass m traveling at speed v, kinetic energy is EsubK = (1/2)m*v2
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potential energy
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Esubp, of an object is the energy that it possesses on account of its position in a filed of force. no specific formula, but an example for gravity is Esubp= mgh (mass m and height h and acceleration of free fall g)
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standard value of g the acceleration of free fall
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g, gravity, = 9.81 m*s-02
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Coulomb potential energy of a particle of charge q1 at a distance or r from another particle of charge q2
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is proportional to the two cahrges and inversely proportional to the distance between them: Ep = (q1q2)/(4π∑0r)
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vacuum permittivity
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∑0, 8.854 x 10-12 J-1C2m-1
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electromagnetic field
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energy such as energy carreid through space by radio waves, light waves, and x-rayes
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electric field
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an oscillating field that generates an electromagnetic field by the acceleration of charged particles
Affects charged particles whether they're still OR moving |
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magnetic field
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an oscillating field that generates an electromagnetic field by the acceleration of charged particles
ONLY affects moving charged particles |
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total energy
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sum of kinetic and potential energy, E = Ek+Ep
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thermal motion
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the chaotic, random motion of atoms and molecules. when a ball hits the earth it is no longer isolated and its energy is dissipated as thermal motion
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law of conservation of energy
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the observation that energy can be neither created nor destroyed
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fundamental charge
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one unit of negative charge = 1.602 x 10-19 C
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α particles
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alpha particles, the positive emitted in streams from some elements
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