Periodic Table: Metals, Nonmetals, and Ions Key Concepts

alkai metals

Group 1A

alkaine earth metals

Group 2

metalloids

group 3a

nonmetals+ two metals

group 4

binary compound

compound between two elements from group 4a-7a with each other of hydrogen (hydrogen bonds with all nonmetals minus noble gases and comp. end in -ide)

metals group 1 ion charge

1+ (cation)

metals group 2 ion charge

2+ (cation)

metals group 3 ion charge

3+ (cation)

group 1-2a and aluminum rule ions

the number of electrons remaining on cations formed is the same number as electrons in an atom of the noble gas that precedes it on periodic table

atomic number

the number of protons (=electrons) in nucleus, denoted by z

mass number

The sum of protons and neutrons in the nucleus of an atom

isotopes

atoms with three same atomic number (protons) but different mass number (diff number of neutrons)

isotopic abundance

% abundance = # of atoms in a given isotope/ total number of atoms of all isotopes of that element x 100-- most isotopic numbers do not have an integer but are close to mass number

metalloids/semi metals

physical properties of metal but chemical properties of a non-metal. in a zigzag shape on periodic table

allotropes

two or more different molecular forms of the same element in the same physical state ex. O2 and O3

transition elements

groups 3-12 on the periodic table

two rows at bottom of periodic table

lanthanides and actinides

group 3a(13)

contain metalloids (Al)

group 4a(14)

nonmetals + two metals

group 5a(15)

contain nonmetals, metalloids, and nonmetals

group 6A(16)

all form sulfur containing compounds

Group 7A(17)

Halogens, all diatomic molecules (Hydrogen, Nitrogen, Fluoride, Oxygen, Iodine, Chlorine, Bromine )

group 8A(18)

noble gases, not reactive

molecular compounds

consist of discrete molecules

ionic compunds are composed of

cations and anions on atoms are groups of atoms (molecules)

monoatomic ions

ions formed from a single atom

metals typically lose on or more electrons (become cations +)

nonmetals typically gain one or more electrons (anions -)

monoatomic cations

atom loses electrons (more protons so postive)

naming monoatomic ions

from group 1,2 that form cations +Al, it's the name of the metal plus word cation

monoatomic anions

more electrons than protons, so negative charge (-)

nonmetals of group 5A-7A monoatomic anions naming rule

form negative charge equal to the group number of the nonmetal -8

Hydrogen ions

can both gain or lose electrons

transition metals (2-13) naming rules

often form more than one type of cation, to specify which ion is involved the charge is indicated by a roman numeral in parenthesis Co^2+= cobalt (II)

monoatomic negative ion

named by adding ide to the stem if the nonmetal element

polyatomic ions

electrically charged particles that consists of two or more atoms bonded together ex. carbonate CO3^2- MOST are oxyanions (OXYGEN WITH NEGATIVE CHARGE (GAIN ELECTRONS))))

most common polyatomic ion

NH4^+, ammonium ion

covalent compounds

between nonmetals and typically share electrons

BrO4^(-1 charge)

Perbromate

BrO3 -1

bromate

BrO2 -1

bromite ion

BrO-

hypobromite ion

ClO4^-1

perchlorate ion

ClO3 -1

chlorate

ClO2 -1

chlorite ion

ClO -1

hypochlorite ion

IO4 -1

periodate ion

IO3 -1

iodate ion

IO2 -1

iodite ion

IO -1

hypoiodite ion

NO3 -1

nitrate ion

NO2 -1

nitrite ion

OH -1

hydroxide ion

CN -1

cyanide ion

SCN -1

thiocyanate ion

C2H3O2 -1

acetate ion

MnO4 -1

permanganate ion

HCO3 -1

bicarbonate (hydrogen carbonate)

CO3 2-

carbonate ion

C8H4O4 2-

Phthalate ion

SO4 2-

sulfate ion

SO3 2-

sulfite

CrO4 2-

chromate

Cr2O7 2-

dichromate ion

C204 2-

oxalate ion

O2 2-

peroxide ion

PO4 3-

phosphate ion

PO3 3-

phosphite ion

AsO4 3-

arsenate ion

HSO4-

hydrogen sulfate (bisulfate)

HPO4 2-

hydrogen phosphate

Hg2 2+

Mercury (I)

NCS- or SCN-

Thiocyanate

group 17 charge

-1 charge

group 16 charge

-2 charge

Group 15 charge

-3 charge

Aluminum charge

3+

zinc charge

Zn2+

Silver charge

Ag+

cadium charge

Cd2+

galium

Ga3+