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72 Cards in this Set
- Front
- Back
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What is the charge of a proton?
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Positive (+)
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What is the charge of a neutron?
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Neutrons have no charge.
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What is the charge of a electron?
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Negative (-)
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Compared to the mass of a proton, an electron is...?
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Smaller than a proton
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Where are protons and neutrons found in an atom?
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The nucleus (nucleons)
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According to the wave mechanical model of the atom, where are electrons found?
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In "clouds" or orbitals around an atoms nucleus.
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The mass number is equal to an atom's number of _____ and ______ added together.
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Protons and neutrons.
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The ______ ______ is equal to the number of protons in the nucleus of an atom.
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Atomic number.
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The _____ __ ______ is equal to:
Mass Number minus atomic number |
Number of neutrons
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______ are atoms with equal numbers of protons , but differ in their neutron numbers.
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Isotopes
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____________ gold foil experiment showed that ____________________
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Ernest Rutherford's /
the atom is mostly empty space with a small, dense, positively- charged nucleus. |
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_________ discovered the electron and developed the "plum pudding" model of the atom.
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J.J Thompson
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______ model of the atom was a solid sphere of matter that was uniform throughout.
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Dalton's
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The ___________ of the atom placed electrons in "planet-like" orbits around the nucleus of an atom.
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Bohr model
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The current, _____________ of the atom has electrons in "clouds" (orbitals) around the nucleus.
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Wave mechanical model
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STP means "___________" and is equal to ____ kelvin and __ atm.
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Standard Temperature and Pressure /
272 kelvin and 1 atm |
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_____ emit energy as light when they jump from higher energy levels back down to lower (_____) energy levels, and ___________ are produced.
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Electrons / ground state / bright line spectra
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_____ are pure substances composed of only one kind of atom.
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Elements
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__________ are substances composed of only one kind of atom. (examples: H2O, NH3, CO2)
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Binary compounds
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___________ are elements that form two atoms molecules in their natural form at STP.
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Diatomic Molecules
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What phrase can you remember to know the diatomic molecules?
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"BrINCIHOF" (Br2, I2, N2, Cl2, H2, O2, F2)
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Air and salt water (solutions) are the best examples of __________.
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Homogeneous mixtures.
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_______ Have discernable components and are not uniform throughout. Some examples include chocolate- chip cookies, vegetable soup, muddy water, etc.
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Heterogeneous mixtures.
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A ______ is the substance being dissolved.
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Solute
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The ______ is the substance that dissolves in the solute.
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Solvent
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The distribution of electrons in an atom is it's ____________
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electron configuration
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_______ are groups of atoms with an overall charge. What table is this on?
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Polyatomic ions / Table E
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_________ are written in front of the formulas of reactants and products in chemical equations. They give us ratios of reactants and products in a balanced chemical equation.
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Coefficients
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___________ do not from new substances. They merely change the appearance of the original material. (the melting of ice)
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Physical changes
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_____________ result in the formation of new substances. (the burning of hydrogen gas to produce water vapor)
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Chemical changes
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_____ are on the left side of the reaction arrow and ______ are on the right.
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Reactants / products
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_____________ absorb heat. The energy value is on the left side of the reaction arrow in a forward reaction.
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Endothermic reactions
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__________ occur when two or more reactants combine to form a single product.
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synthesis reactions
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________ occur when a single reactant forms two or more products.
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Decomposition reactions
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____________ occur when one element replaces another element in a compound.
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Single replacement reactions
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_____________ occur when two compounds react to form two new compounds.
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Double replacement reactions
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law of Conservations of Mass?
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The masses of the reactants in a chemical equation is always equal to the masses of the products.
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The particles in a _____ are rigidly held together.
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Solid
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_____ have a definite shape and volume.
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Solids
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______ have closely-spaced particles that easily slide past one another.
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Liquids
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______ have no definite shape, but do have a definite volume.
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Liquids
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______ have widely-spaced particles that are in random motion.
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Gasses
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______ are easily compressed and have no definite shape or volume.
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Gasses
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Substances that ______ turn from a solid directly into a gas.
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Sublime
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How do you convert degrees celsius to degrees kelvin?
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Degrees celsius + 273
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What formula would you use to calculate heat absorbed / released by substances questions? What does each thing in the equation stand for?
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q=mcΔt
q= heat absorbed or released (joules) m= mass of substance in grams c= specific heat capacity of substance (J/g times degrees celsius) ..... for water it's 4.18 Δt= temperature change in degrees celsius |
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The heat absorbed or released when 1 gram of a substance changes between the solid and liquid phases is the substance's ______.
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Heat of fusion. (334 J/g for water)
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The heat absorbed or released when 1 gram of a substance changes between the liquid and gaseous phases is the substances _________.
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Heat of vaporization. (2260 J/g for water)
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As the pressure on a gas increases, the _______ decreases proportionally.
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Volume
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As the pressure on a gas increases, the _______ increases.
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Temperature
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As the temperature of a gas increases, the _____ increases.
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Volume
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_______ particles have volume and are attracted to one another, and thus do not always behave like ______.
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Real gas / ideal gasses
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Real gasses behave more like ideal gasses at ____ pressures and _____ temperatures.
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Low pressures and high temperatures.
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_______ separates mixtures with different boiling points
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Distillation
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_______ separates mixtures of solids and liquids
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Filtration
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__________ can also be used to separate mixtures of liquids and mixtures of gasses.
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Chromatography
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________ states that the properties of elements are periodic functions of their atomic numbers.
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The periodic law
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______ are horizontal rows on the Periodic Table.
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Periods
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_____ are vertical columns on the Periodic Table.
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Groups
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____ are found left of the staircase on the Periodic table, and ______ are above it, and _______ border it.
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Metals / nonmetals / metalloids
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Characteristics of Metals
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Malleable / ductile / lustrous / god conductors of heat and electricity / low ionization energy and electronegativity / tend to form positive ions
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Characteristics of Nonmetals
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Brittle when solid / mostly gases at STP / dull / good insulators / high ionization energy and electronegativity / tend to form negative ions
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______ (group 18) are inert and stable due to the fact that their valence level of electrons is completely filled.
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Noble Gasses
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________ increases as you go up to the right on the Periodic Table
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Ionization energy
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________ decrease left to right across a period due to increasing nuclear charge.
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Atomic radii
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_______ increase as you go down a group.
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Atomic radii
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_________ is a measure of an element's attraction for electrons. It also increases as you go up to the right on the Periodic Table
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Electronegativity
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The elements in Group 1 are the _______.
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Alkali metals
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The elements in Group 2 are the ________.
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Alkaline earth metals
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The elements in Group 17 are the ________.
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Halogens
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The elements in Group 18 are the ________.
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Noble gasses
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The last digit of an element's group number is equal to it's _________.
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Number of valence electrons
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