AP Chemistry Vocabulary

4

F (electronegativity)

2.1

H (electronegativity)

3.5

O (electronegativity)

3.0

N (electronegativity)

3.2

Cl (electronegativity)

2.5

S (electronegativity)

2.5

C (electronegativity)

2.8

Br (electronegativity)

180

the approximate bond angle for a linear structure

120

the approximate bond angle for a trigonal planar structure

120

the approximate bond angle for a bent structure

109.5

the approximate bond angle for a tetrahedral structure

109.5

the approximate bond angle for a trigonal pyramidal structure

109.5

the approximate bond angle for a bent structure with 4 electron domains

90, 120

the approximate bond angle for a trigonal bipyramidal structure

90, 120

the approximate bond angle for a see-saw structure

90

the approximate bond angle for a t-structure

90, 90

the approximate bond angle for an octahedral structure

90, 90

the approximate bond angle for a square pyramidal structure

90

the approximate bond angle for a square planar structure

linear

the name for a geometry with 2 bonding domains and 0 nonbonding domains

trigonal planar

the name for a geometry with 3 bonding domains and 0 nonbonding domains

bent

the name for a geometry with 2 bonding domains and 1 nonbonding domain

tetrahedral

the name for a geometry with 4 bonding domains and 0 nonbonding domains

trigonal pyramidal

the name for a geometry with 3 bonding domains and 1 nonbonding domain

bent

the name for a geometry with 2 bonding domains and 2 nonbonding domains

trigonal bipyramidal

the name for a geometry with 5 bonding domains and 0 nonbonding domains

see-saw

the name for a geometry with 4 bonding domains and 1 nonbonding domain

t-structure

the name for a geometry with 3 bonding domains and 2 nonbonding domains

linear

the name for a geometry with 2 bonding domains and 3 nonbonding domains

octahedral

the name for a geometry with 6 bonding domains and 0 nonbonding domains

square pyramidal

the name for a geometry with 5 bonding domains and 1 nonbonding domain

square planar

the name for a geometry with 4 bonding domains and 2 nonbonding domains

molar mass

the mass of one mole of a substance

isotopes

each form of the same element that contains equal numbers of protons but different numbers of neutrons in the nucleus

average atomic mass

average mass of an element based on the percent abundance of each isotope in nature

chemical formula

identification of a particular substance by its combination of atoms

molecular formula

chemical formula that has the exact number of atoms for each element of the molecule

empirical formula

chemical formula with the lowest whole number ratio of atoms in the compound

law of definite proportions

the ratio of the masses of the constituent elements in any pure sample of a compound or molecule is always the same

hydrate

an ionic compound that has incorporated a number of H2O molecules

Aufbau’s Principle

when determining what energy level an electron will be found in, it must be in the lowest shell available

electron configuration

a way of depicting in which shells and subshells all of the electrons in an atom will be found

Coulomb’s Law

can be used to rationalize ionization energies

orbital diagrams

an alternative way of depicting in which orbitals electrons of an atom or ion are in

Pauli’s Exclusion Principle

electrons have a spin state referred to as “spin up” or “spin down”

Hund’s Rule

when placing electrons into degenerate (equal in energy) suborbitals, you must place one electron in each before adding a second electron in any of them

isoelectric

same number of electrons

ionzation energy

the amount of energy it takes to remove an electron

photoelectron spectroscopy

a tool for determining element and multiple ionization energies

effective nuclear charge

the amount of pull the valence electrons feel from the nucleus

increasing left to right

periodic trend for effective nuclear charge

increasing diagonally to top right

periodic trend for ionization energy

decreasing diagonally to top right

periodic trend for atomic radius

electron affinity

the amount of energy gained by gaining an electron

increasing diagonally to top right

periodic trend for electron affinity

electronegativity

how strongly an atom pulls electrons of a covalent bond towards itself

electron-electron repulsion

the reason why N has a higher ionization than O

only one electron in p orbital

the reason why Be, Mg, and column 12 have higher ionization energies than B, Al, and column 13

cations

positively charged ions

anions

negatively charged ions

cation, anion

order that ions are written in ionic compounds

covalent bond

two atoms sharing electrons so that both ahve a full octet

ionic bond

“lattice energy;” array of interactions between cations and anions that maximizes coulombic attraction while minimizing coulombic repulsions

metallic bond

the valence electrons become a “sea of electrons” in this type of bond

IMFs

bonds between molcules or atoms

ionic solids

properties include: 3-d array, brittle, conduct electricity in liquid form or when aqueous, low boiling point and melting point

substitutional alloy

alloy in which atoms that are similar in size are randomly distributed

london dispersion forces

coulombic interactions, weakest IMG; always present

polarizability

coulombic interaction slightly larger than london dipersion, present whenever a larger atom (period 3 and lower) is present

dipole-induced dipole

interaction between a molecule with a dipole moment and one without

dipole-dipole

interaction between two molecules when both have dipole moments

ion-dipole

force of attraction between an ion and a molecule with a dipole moment

hydrogen bonding

strong IMF that forms between an atom that is bonded to an N, O, or F and another atom with at least one lone pair of electrons

covalent networks

properties include: only non-metals, high melting point, no IMFs, rigid and hard

molecular solid

properties include: low melting point, good insulators

metallic solids

properties include: conductors of electricity and heat, high melting and boiling points; malleable and ductile

solid

properties include: can be crystalline or amorphous; motion is greatly limited; definite shape and volume

liquids

properties include: particles close together, constantly in motion, arrangement and movement influenced by IMFs, no definite shape, definite volume

gases

properties include: made up of particles that are in constant motion, frequencey of collisions is dependent on temperature, pressure, and volume; no definite shape or volume

zero degrees celsius, 1 atm

conditions of STP

at low temperatures and high pressures

when do gases deviate from the ideal gas law

mobile phase

nonpolar phase of chromatography

stationary phase

polar phase of chromatography

distillation

using different boiling points and condensing each component to separate a mixture of liquids

microwave

radiation that causes rotations of particles

infrared

radiation that causes vibrations of particles

UV/visible light

radiation that causes particles to move to higher energy levels

all, certain wavelengths

metal reacts with _____ light, while ionic/covalent substances react with _______ of light.

NO3-

nitrate

NO2-

nitrite

ClO4-

perchlorate

ClO3-

chlorate

ClO2-

chloite

ClO-

hypochlorite

OH-

hydroxide

CN-

cyanide

CH3COO-

acetate

SO42-

sulfate

SO32-

sulfite