Chemistry Exam Review

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volume

Back 1

L x W x H

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potential energy

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stored energy

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kinetic energy

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energy of movement

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radiant energy

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energy in motion

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true or false: zeros used for spacing the decimal point are significant.

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false

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Law of Conservation of Energy

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Energy changes form

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Law of conservation of matter

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All matter/atoms are the same, never has changed, never will change.

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Law of conservation of mass-energy

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Matter gets transformed into energy and vice versa

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List five indications of chemical changes

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burns, color, bubbles, change in heat/energy change, explosions, rust, smoke

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"ide" means the chemical is --charged

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negatively

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"ium" means the chemical is -- charged

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positively

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Bromide

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Br-1

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Sulfide

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S2-

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Sulfur

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S

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Nitride

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N3-

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Chloride

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Cl-

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Oxide

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O2-

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Oxygen

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O2+

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Phosphide

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P3-

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Phosphorous

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P

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Flouride

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F-

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Magnesium

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Mg2+

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Aluminum

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Al3+

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iodide

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I-

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Phosphate

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Po4 up 3-

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Ammonium

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NH4+

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Sulfate

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SO4 up 2-

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Iron II

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Fe2+

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Iron III

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Fe3+

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Nitrate

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NO3-

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Nickel II

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Ni2+

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Potassium

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K+

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Zinc

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Zn2+

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Sodium

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Na+

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Acetate

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CH3COO-

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Copper I

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Cu+

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Copper II

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Cu2+

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Calcium

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Ca2+

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Hydrogen

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H+; when diatomic H2+

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Carbonate

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CO3 up 2-

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Lithium

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Li+

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Silver

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Ag+

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Hypochlorite

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OCl-

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daltons atomic theory of matter

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1. each element is made of extremely small particles (atoms)
2. All atoms in a given element are identical, but they differ from those of any other element
3. Atoms are neither created nor destroyed in any chemical reaction
4. A given compound always has the same relative numbers and kind of atoms

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atoms combine to form

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substances

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atoms are made of particles that have an--

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electric charge

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ion

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an atom that is electrically charged (+/-)

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cation

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an ion with a + charge

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anion

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an ion with a - charge

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cobalt III

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Co3+

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cobalt II

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Co2+

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ions of different elements combine to form

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ionic compound

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chemical formula

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tells us what kind of atoms/ions and how many/ratio

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compounds are electronically

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neutral

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the formula of an ionic compound should be

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reduced to give the smallest whole number ratio of ions

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process by which a substance or substances are converted into different substances with new chemical and physical properties

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chemical reaction

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list five examples of chemical reactions

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metal>rust
dough>bread
leaves changing color
hair perm

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what happens in a chemical reaction?

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reactants are converted into products

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a chemical equation describes:

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exactly what happens in a chemical reaction

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list the five types of chemical reactions

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1. Direct Combination/Synthesis
2. Decomposition
3. Single-Replacement
4. Double-Replacement
5. Combustion

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Atoms that were -- replace other atoms that were --; atoms that were -- replace other atoms that were --!

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For single and double replacement reactions, --cations, cations, anions, anions

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when reactants react in a combustion rection, they always give off

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CO2 and H20

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atomic mass

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the mass of a single atom (not in grams) given/measures in amu's (atomic mass unit)
atomic mass of any atom is based on the mass of a carbon atom
it's at the bottom of the square on periodic table

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formula mass

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sum of masses of all atoms in a compound

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mole

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the number of atoms of the element=the number of atoms in 12.0 g carbon-12

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molar mass

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the mass of a mole of a substance, or the mass of 6.02 x 10 up 23 particles of that substance

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molar mass is the same thing as:

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atomic mass

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for a compound, molar mass is the same thing as:

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formula mass

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converting from mass-moles

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molar mass (g/mol)

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converting from volume to moles

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22.4 Liters (only at STP)

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converting from particles to moles

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6.02 x 10 up 23

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moles-moles conversion

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ratio of moles in the equation

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at a temperature of 0 degrees celcius, and a pressure of 1 atmosphere, 1 mole of any gas has a volume of

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22.4 L...this is STP which stands for standard temperature and pressure

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percent composition

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the percent of the mass of compound made up by each element

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empirical formula

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formula that gives us the lowest whole number ratio of atoms in a covalent compound

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molecular formula

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formula giving actual numer of atoms in a covalent compound; not necessarily lowest terms
*in order to find molecular you have to find empirical

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using chemical formulas and equations to figure out amounts of substances that undergo chemical changes

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stoichiometry

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matter is neither created nor destroyed, atoms cannot be gained or lost, even during a chemical reaction nothing is destroyed it just changes, the total mass of the reactants in a chemical reaction must equal the mass of the products.

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law of conservation of matter

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balanced chemical equations give us both the relative number of -- and the relative number of ---

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--atoms/particles---moles

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the reactant thats used up in a chemical reaction

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limiting reagent

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the reactant that's left over in a chemical reaction

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excess reagent

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the limiting reagent determines

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how much product is formed!

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in chemical reactions, atoms are rearaanged and new substances are formed. based on these arrangements, chemical reactions can either absorb or release--

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energy

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the energy exchanged between objects due to a difference in temperature

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heat

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study of changes in heat that accompany chemical reactions (chemistry having to do with heat)

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thermochemistry

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exothermic reaction

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reaction that gives off or releases heat into the surroundings (-)

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endothermic reaction

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reaction that takes in or absorbs heat from the surroundings

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measure of heat absorbed or released by a chemical reaction occurring at constant pressure

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enthalpy change

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enthalpy change for reactants in their standard state being converted to products in standard state.

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standard enthalpy change

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standard state (for enthalpy change)

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1 atm and 25 degrees celcius

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caloric theory

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early scientists thought heat was an invisible, weightless liquid that flowed from hotter objects to cooler objects

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kinetic theory

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currently accepted; heat comes from the motion and vibrations of particles of matter.
heat is the transfer of kinetic energy (of motion) from a hotter object to a cooler one (at the atomic level so it's not visible)

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an exothermic reaction releases heat, so the temperature of the surroundings

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increase

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an endothermic reaction absorbs heat, so the temperature of the surroundings

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decreases

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calorimetry

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the study of heat flowand heat measurement, allows scientists to measure the standard enthalpy change by using calorimeter.

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specific heat

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the amount of heat required to raise 1gram of a substance by 1 degree celcius

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describe a proton and its (charges, mass, and location)

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charge of +1
mass of 1 amu
location- in the nucleus

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describe an electron (charge, mass, location)

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-1 charge
mass, so small we ignore
located outside nucleus

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neutrons
describe location, charge, mass

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no charge, neutral
mass about 1 amu
located inside nucleus

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mass number

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the sum of the protons and neutrons
found by taking the # protons and adding to the # neutrons

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how do you know how many electrons there are?

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there are the same number of electrons as neutrons, unless it has a charge in which case if it's positive there is one more electron and if it's negative that means there is one less

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recall what you know about the electron

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electrons only have specific energies
electrons have wavelike properties
we cant know the location and where the electron is going at the same time

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What does the quantum mechanical model do?

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describes the electron using the idea of ELECTRON DENSITY

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region around the nucleus where there is a high probability of finding an electron of a given energy.

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orbital

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gives a definite electron path

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orbit

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lowest energy orbital to highest in letters; number of orbitals each one holds, and shapes

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s, p, d, f
1 3 5 7
s=sphere
p=dumbbell
d, f =complex

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if the quantum number/principal energy level is n=3, how many sublevels are there?

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3

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describe the characteristics of metals

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location: left of zigzag
properties: shiny
good conductors of energy
solids at room temperature
malleable (can be hammered into a thin sheet)
ductile (can be pulled into thin wires)

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properties of nonmetals

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right of zigzag
not shiny
poor conductors of heat and electricity
may be solids, liquids, or gases
neither melleable, or ductile

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semimetals

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touching zz line

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valence electrons

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electrons that occupy the highest principle energy level/have highest quantum number level, determine chemical reactivity of the atom

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periodic law

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when the elements are arrangedin order of increasing atomic number, we can see the trends in their chemical and physical properties

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groups

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vertical columns in periodic table

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periods

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horizontal rows in periodic table

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alkali metals, alkaline earth metals, halogens, noble gases

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groups in periodic table

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atomic radius

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distance from center of nucleus to outermost electron

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as you move down a column

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atomic radius increases
ionization energy decreases
electronegativity decreases

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a cation is -- than the corresponding neutral atom

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because it has lost an electron making it positive, it is --smaller

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an anion is -- than its corresponding neutral atom

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because it has gained an electron, it is larger than its corresponding neutral atom

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metals form

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cations

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nonmetals form

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anions

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ionization energy

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energy required to remove an electron from and atom or an ion

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as you move across a period, the

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atomic radius decreases
ionization energy increases
electronegativity increases

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electron affinity

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the energy abosorbed (required) or released for an atom or ion to gain an electron

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the closer an atom is to filling its valence shell, the --its electron affinity

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greater; because more energy is released and it wants an electrom

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the atom's ability to attract electrons

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electronegativity

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electrons are only allowed to have certain - corresponding to different amounts of -- (ie. the energy of an electron is --)

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orbits, energies, quantized.

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when an electron is falling back down to its ground state, -- is emitted

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light

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frequency determines the -- of the light emitted when an electron drops back down to its ground state

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color

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excited state

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higher energy level so in order for an electron to be in an Excited state, something would have to happen to it (further from nucleus, higher energy)

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DEBROGLIE and matter waves

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he predicted that all moving objects exhibit wavelike behavior; electrons have wavelike properties
he related mass-wavelength

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HEISENBERG uncertainty principle

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you cannot know the precise location of an object and exactly where it is going at the same time
makes no difference for larger objects

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how does the heisenberg uncertainty principle affect a tiny particle like an electron

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to locate an electron, you have to shine light on it, and by doing so, by hitting it with photons, its path is being changed

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height of wave

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amplitude

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wavelength

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distance from crest to crest

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how fast the wave moves back and forth in a given amount of time

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frequency

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less wavelength =

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larger frequency

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larger wavelength=

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smaller frequency

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speed

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how fast the wave moves through space

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photons-

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light particles carrying small amounts of energy

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photoelectric effect-

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when light was shined on certain metals, electrons were emitted

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light is dual natured it is:

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wave and particle

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red- what level energy

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low energy, lower frequency

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violet- what level energy

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higher energy, higher frequency

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planck's quantum theory/equation

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objects can only abosorb or release energy in fixed amounts, called quanta
e=hv relates energy of wave to frequency

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the aufbau principle

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electrons are put into the lowest enerfy orbitals one at a time until all of the electrons are accounted for

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the number of electrons in a neutral atom= # of protons =

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atomic #

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list the diagonal rule

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1s, 2s, 2p, 3s, 3p, 3d, 4s, 4p, 4d, 4f, 5s, 5p, 5d, 5f, 6s, 6p, 6d, 6f

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the pauli exclusion principle

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when two electrons are in the same orbital, they will spin in opposite directions (have opposite spins) two arrows, one goes up, one down

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hund's rule

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in a given sublevel, one electron will go into each orbital before beginning to pair