Chemistry Test 2

Na^+

sodium ion

Mg²+

magnesium ion

Al³+

aluminum ion

Ag³+

silver ion

Fe²+

iron ion

Cu^+

copper ion

K^+

potassium ion

Ca²+

calcium ion

Zn²+

zinc ion

NH4^+

ammonium ion

Fe³+

iron ion

Cu²+

copper ion

F^-

Fluoride ion

Br^-

Bromine ion

S²-

sulfur ion

NO3^-

nitrate

HCO3^-

Bicarbonate

SO4²-

Sulfate

Cl^-

chlorine ion

I^-

iodine ion

O²-

oxide ion

CO3²-

carbonate

OH^-

hydroxide ion

PO4³-

phosphate ion

atomic number

number of protons

mass number

number of protons plus neutrons

radioisotopes

an element with the correct number of protons but a different number of neutrons

stable nuclei

the correct number of protons and neutrons for an element

unstable nuclei

a correct number of protons but an incorrect number of neutrons

Alpha particles

least potent radiation, don’t breathe in

alpha particle decay formula

mass change by 4 and protons by 2

beta particles

more potent than alpha

beta decay formula

no mass change but gain one proton

positrons

more potent than beta

positron formula

proton into neutron element -1

gamma radiation

most potent long term decay

positron emmission

activity x branching ratio = positron emission rate (MBq)

gamma radiation formula

no element or mass change

half life

divide by two to get the half lives

cation

positive ion

anion

negative charge

binary ionic compounds

metal + nonmetal with -ide suffix

variable change metals

transition metals with roman numerals in name

naming compounds with polyatomic ions

first element than the polyatomic ion no suffix change

ionic compounds

metal and non-metal spectator in lewis structure

covalent bonds

two non-metals bonded in lewis structure

1

mono

2

di

3

tri

4

tetra

5

penta

6

hexa

7

hepta

8

octa

9

nona

electron group geometry

considers all electron pairs lone and bonded

molecular geometry

focuses only on the positioning of electrons, ignores lone pairs

linear

even distribution of electrons straight line

trigonal planar egg

spatial arrangement including lone pairs flat

trigonal planar molecular geometry

only bonded pairs flat and 3 around atom

tetrahedral

4 around central atom

bent

bonded to two other atoms central atom surrounded by one or two lone pairs

electronegativity

increases left to right and down to up most being fluorine

polar compounds

nonsymmetrical distribution of electrons

non-polar compounds

even distribution of electrons

dipole dipole

like a magnet positive and negative, second weakest bond

dispersion

weakest bonding

ionic bonds

strongest bond

covalent bonds

second strongest bond

hydrogen bond

third strongest bond