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CH 101: EXAM 1
atom |
The smallest particle of an element that retains the properties of the element
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mole |
6.02 * 10^23 items. Number of molecules/atoms in a sample of a compound/element that has a mass equal to its molecular/atomic mass
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Avogadro's Number |
6.02 * 10^23, the number of items in a mole
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molar mass |
molar mass The mass of one mole of substance
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conversion factor |
Fraction used to convert one quantity in one unit to an equivalent quantity in another unit
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potential energy |
Energy due to position
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Coulomb's Law |
E = q1q1/r
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"lower energy" |
More negative
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cathode ray |
a stream of electrons produced at the negative electrode of a tube containing a gas at low pressure
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subatomic particle |
Particles smaller than an atom (Electrons, Protons, Neutrons)
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electron |
A subatomic particle found outside the nucleus. It carries a -1 charge and has a mass of 5 * 10^-4 amu
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proton |
A subatomic particle found in the nucleus. It carries a +1 charge and has a mass of ~1 amu
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neutron |
A subatomic particle found in the nucleus. It carries no charge and has a mass of ~1 amu
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ion |
A charged species
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cation |
A positively charged species because it contains fewer electrons than protons
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anion |
A negatively charged species because it contains more electrons than protons
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atomic number |
The number of protons in the nucleus. It is the number that identifies the atom
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mass number |
The number of protons plus the number of neutrons in the nucleus
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isotope |
Atoms with the same atomic number but different mass numbers
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average atomic mass |
weighted average of the atomic masses for the isotopes of an element
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period |
A horizontal row in the periodic table. The properties of the elements in a period vary gradually across the period
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group |
A vertical column in the periodic table. The elements in a group have similar properties
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metal |
A material that is shiny, malleable, and a good conductor of electricity. Elements that are metals lie on the left side of the periodic chart and represent about 80% of the elements. Metals react with nonmetals to form ionic compounds
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non-metal |
Elements that are gases, liquids, or solids that are dull, brittle, and poor conductors of electricity. Nonmetals lie on the right side of the periodic chart. Nonmetals react with one another to form covalent compounds or with metals to form ionic compounds
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metalloid |
Have properties intermediate between the metals and nonmetals.
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alkali metal |
An element that belongs to Group 1A
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alkaline earth metal |
An element that belongs to Group 2A
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halogen |
An element that belongs to Group 7A
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noble gas |
An element that belongs to Group 8A
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spectrum |
Radiant energy arranged in order of its frequency or wavelength
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wavelength |
The distance between a point on a wave and the corresponding point on the next wave
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speed of light |
3e8
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frequency |
The number of oscillations per second that a wave undergoes
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photoelectric effect |
The emission of electrons from a metal when light shines on the metal
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quantized |
exists in discrete amounts
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Bohr model |
model of the atom in which electrons move rapidly around the nucleus in paths called orbits
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emission |
Emission of a photon decreases the energy of an atom or a molecule by the energy of the photon (hν). The energy of the photon equals the energy difference between two energy levels in the molecule or atom
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absorption |
Absorption of a photon increases the energy of an atom or a molecule by the energy of the photon (hν). A photon can be absorbed only if its energy matches the energy difference between two energy levels in the atom or molecule
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wavefunction |
A function that contains all of the information about an electron in an atom
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orbital |
A solution to the wave equation. It is most commonly used to refer to the region to which an electron is confined most of the time. In other words, it shows the electron density of the electron(s) that it contains
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s-orbital |
An atomic orbital that is spherical and symmetrical, centered on the nucleus
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p-orbital |
An atomic orbital that is composed of two lobes located symmetrically about the nucleus and contains a node
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level |
An allowed energy designated by a quantum number. The level of an electron in an atom is designated by the n quantum number
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sublevel |
Specified by the n and l quantum numbers, it dictates the energy of the electron and the size and shape of the orbital
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standing wave |
A wave that appears to stand in one place
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node |
A point of zero amplitude on a standing wave
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orbital energy diagram |
Shows the orbitals on an energy axis. Each horizontal line represents an orbital.
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unpaired electron |
Electrons that do not have a corresponding spin to pair with
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Hund's Rule |
The number of electrons with identical spin is maximized when filling the orbitals of a sublevel
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s-block |
Contains all elements in groups 1A through 2A, and He. Can hold up to 2 electrons
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p-block |
Contains all elements (other than He) in groups 3A through 8A. Can hold up to 10 electrons
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d-block |
Contains all elements in groups 3B through 2B. Can hold up to 6 electrons
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f-block |
Can hold up to 14 electrons; the f-block is 14 elements wide
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valence electron configuration |
A listing of the occupied sublevels that contain valence electrons and the number of valence electrons that they contain
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electron configuration |
A listing of the occupied sublevels and the number of electrons that they contain
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atomic radius |
One-half the separation between two atoms that make contact in the unit cell of a metal atom
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shielding |
The amount by which the nuclear charge experienced by an electron is reduced by the negative charge of other electrons
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effective nuclear charge |
The nuclear charge experienced by an electron. Zeff for a valence electron is less than the full nuclear charge due to shielding by the other electrons.
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ionization energy |
The energy required to remove an electron from an atom or molecule
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electron affinity |
The energy required to remove a valence electron from an anion
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electronegativity |
A relative measure of the ability of an atom to attract bonding electrons to itself. Atoms with high electronegativities have unfilled orbitals that are low in energy
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Quantum Model |
Numbers (usually integers) that designate the allowed states. (In this course, we consider quantum numbers for electrons only)
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Greek prefix 1 |
mono
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Greek prefix 2 |
di
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Greek prefix 3 |
tri
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Greek prefix 4 |
tetra
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Greek prefix 5 |
penta
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Greek prefix 6 |
hexa
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Greek prefix 7 |
hepta
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Greek prefix 8 |
octa
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How many electrons does H like to have around it? |
2
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SP = |
1/2 [ ER - VE ]
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Lewis structure |
A representation of a molecule that shows all of the valence electrons as dots. The dots are usually in pairs that represent bonding and nonbonding pairs. Bonding pairs are often represented by lines
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shared (bonding) pairs |
Pairs of bonding electrons
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lone (non-bonding) pairs |
Pairs of nonbonding electrons
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valence electrons |
The outermost electrons that dictate the properties of the atom and are involved in chemical bonding. They reside in the outermost s sublevel and any unfilled sublevels
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bond order |
The number of shared pairs in a bond
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octet rule |
Atoms (except for H) strive to obtain an octet (eight) valence electrons in their molecules.
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