chem semester one

deci-

(d) 10^-1

tera-

(T) 10^12

giga-

(G) 10^9

kilo-

(k) 10^3

femto-

(f) 10^-15

centi-

(c) 10^-2

deca

(da) 10^1

milli-

(m) 10^-3

micro-

(μ) 10^-6

nano-

(n) 10^-9

mega

(M) 10^6

pico-

(p) 10^-12

hecto-

(h) 10^2

ionic bonds

bonds between metals and nonmetals (valence electrons are completely transferred between atoms, the electronegativity of one atom is much different from the other atom it is bonding to, so electrons completely "change hands", either positive or negative charges are produced on the atom)

covalent bonds

bonds between nonmetals and nonmetals (valence electrons are shared between atoms, the electronegativity of an atom is close to the other it is bonding to, so electrons are shared, no charges are produced because complete ownership of electrons is not established unless it is polar)

what side of the staircase are metals

left

what side of the staircase are nonmetals

right (except for hydrogen)

do metals tend to oxidize or reduce

oxidize

do nonmetals tend to oxidize or reduce

reduce

do metals form to cations or anions

cations

do nonmetals form to cations or anions

anions

what ends in the suffix -ide in ionic compounds (cations or anions)

anion (except for in polyatomic ions)

what happens when a polyatomic ion gains an electron

prefix per- added

what happens when a polyatomic ion loses an electron

suffix -ite replaces -ate

what happens when a polyatomic ion loses two electrons

prefix hypo- added (as well as suffix -ite replaces -ate)

non-polar covalent bond

bonding electrons shared equally between two atoms creating no charges on atoms (absolute value of different of energy is less than 0.5)

polar covalent bond

bonding electrons shared unequally between two atoms creating partial charges on atoms (absolute value of different of energy is greater than or equal to 0.5)

three steps of naming covalent compounds

1. turn subscript into a prefix 2. turn symbol into the element name 3. change second elements suffix to -ide

prefix for an atom with one as a subscript

mono (only used for the second element)

prefix for an atom with two as a subscript

di

prefix for an atom with three as a subscript

tri

prefix for an atom with four as a subscript

tetra

prefix for an atom with five as a subscript

penta

prefix for an atom with six as a subscript

hexa

prefix for an atom with seven as a subscript

hepta

prefix for an atom with eight as a subscript

octa

prefix for an atom with nine as a subscript

nona

prefix for an atom with ten as a subscript

deca

steric number

number of bonded atoms and lone pairs on the central atom

what determines molecular geometry

number of lone pairs

relationship between lone pairs and repulsion

direct

where do you put extra electrons when drawing a Lewis Structure

on the middle atom

what is a dipole created by

separation of the partial charges in a polar bond

net dipole movement

region of space in which there is a partial negative charge/dipole and partial positive charge/dipole in a polar molecule

what two things do dipole moments have

magnitude and direction

non-polar molecules

molecules whose atoms have symmetrical shapes and bonded atoms with the same electronegativity

two kinds of forces/attractions that operate in a molecule

intramolecular and intermolecular

intramolecular forces

(IMFS) forces that hold atoms together within a molecule (represented with dotted line)

intermolecular forces

(IMFS) forces that exist between molecules (polarity determines the type of intermolecular force within each molecule)

dipole-dipole force

electrostatic attraction between opposite poles of polar compounds

hydrogen bonding

strong kind of dipole-dipole interaction that occurs between a H atom bonded to a N, O, or F atom (not actual bond, but attraction)

London dispersion forces

(LDF) temporary and weak attraction force that all molecules have that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles (induced dipoles caused by polarized electrons clouds)

what do London dispersion forces depend on

size of the atom's electron cloud and the size and shape of the non-polar molecule (hydrocarbons are non-polar molecules)

are asymmetrical molecules always polar or non-polar

polar

matter

anything that has mass and takes up space

mass

measure of how much material is within an object

volume

amount of space an object takes up

pure substance

sample of matter with both definite and constant composition and distinct chemical properties

heterogeneous mixture

mixture with non-uniform composition

mixture

two or more substances are combined and each substance stays the same

homogeneous mixture (solution)

mixture has some composition and appearance throughout

element

substance that cannot be separated into simple substances by chemical means

compound

combination of two or more elements which can be separated by chemical means but cannot be separated any other way

kinetic energy

energy associated with an objects motion

potential energy

energy associated with an objects position and attractive forces

diatomic molecules

HOFBrINCl

ionic compounds (formula units)

compound composed of a metal and a non-metal

covalent compounds (molecules)

compound composed of two non-metals

density

mass per unit of volume

physical property

property that can be observed without changing the composition of the substance

conductivity

ability to allow heat or electricity to pass through a material

ductility

ability of some metals to be pulled into wires

malleability

ability of some metals to be hammered or rolled into thin sheets

luster

having a shiny appearance or reflecting light

viscosity

resistance of a liquid to flow

chemical property

property indicating if a substance is able to change into other substances with new and different properties

extensive property

property that depends on the amount of the matter being measured

intensive property

property that does not depend on the amount of the substance present

pressure

measure of force over an area of a substance (atm)

triple point

point at which solids, liquids, and gases can coexist

normal boiling point

temperature at which the vapor pressure of a liquid is equal to standard atmospheric pressure

standard atmospheric pressure

1 atm

standard temperature

273 K or 0 C

normal melting point

temperature at which the vapor pressure of the solid and the vapor pressure of the liquid are equal

critical temperature

temperature above which the substance cannot exist in the liquid state

critical pressure

lowest pressure at which the substance can exist as a liquid at the critical temperature

evolution of gas

usually indicated by bubbles

formation of color

when a different color or odor appears suddenly, this usually means a new substance with new properties has formed

precipitate

formation of a solid substance

temperature change

if a new substance becomes warmer in temperature even though no heat is being

production of light

sometimes during a chemical change light is given off

which way are groups on the periodic table

vertical (up and down)

which way are periods on the periodic table

horizontal (left and right)

average atomic mass

all of the masses of naturally occurring elements and is located beneath the element symbol on the periodic table

oxidation number

likely charge an element will make as an ion

what makes up the overall size of the atom

electrons

isotope

atoms of the same element with different amounts of neutrons (or mass numbers)

equation to find average atomic mass of an element

((abundance % x mass) + (abundance % x mass)...)/100

anion

negatively charged ion

cation

positively charged ion