Periodic table and Memorization

Metals areas in the periodic table and characteristics

• comprise most of the elements and usually lose electrons when involved in chemical reactions

• good electrical and thermal conductors

Nonmetals in the periodic table and characteristics

• are located near the top right of the periodic table

• usually gain electrons from metals and share electrons with other nonmetals in a reaction

Metalloids on the periodic table and characteristics

• can swing both ways

• can be found in the region on the table between the metals and the non metals

• Boron, silicon, germanium, arsenic, antimony, and tellurium

Groups vs periods

• groups

  • Vertical lines on the Periodic table

  • Elements in the same group usually have similar chemical and physical properties

• Periods

  • Rows in the periodic table

group 1A

• Alkali metals

• solid at room temp, react violently with water

• always +1

• hydrogen here doesn’t count

Group 2A

• alkaline earth metals

• Solid at room temp

• React vigorously with oxygen

• always +2

Groups 3-12

• transition metals

• Variable charge → Roman numerals are required

• You back-calculate the charge from the anion

group 13

• AL is always +3

• B is metalloid

Group 15

Pnictogens

Anion charge −3: nitride N³⁻, phosphide P³⁻

Group 16

Chalcogens

Anion charge −2: oxide O²⁻, sulfide S²⁻, selenide Se²⁻.

O is −2 in almost everything (exceptions: peroxides O₂²⁻ where it's −1, and OF₂ where it's +2).

Group 17 or 7A

Halogens

Anion charge −1: fluoride, chloride, bromide, iodide.

Diatomic as elements (F₂, Cl₂, Br₂, I₂).

mostly gas at room temp

Forms salts when bonded with a metal

Group 18 or 8A

Noble gases

Gases at room temp

Diatomic molecules

Have (H2)

No (N2)

Fear (F2)

Of (O2)

Ice (I2)

Cold (CL2)

Beer (Br2)

chromous

Cr²+

chromium(II)

Chromic

Cr³+

chromium(III)

Cuprous

CU^1+

Copper(I)

Curpric

Cu²+

copper(II)

Ferrous

Fe²+

Iron(II)

Ferric

Fe³+
Iron(III)

mercurous

Hg2²+

Mercury(I)

Mercuric

Hg²+

Mercury(II)

Stannous

Sn²+
tin(II)

Plumbous

Pb²+

Plumbic

Pb^4+

Stannic

Sn^4+

Tips for special transition metal naming for special ones

Pattern 1: The suffix always means the same thing

• -ous is the lower charge

• -ic is the higher charge

Pattern 2: The change gap depends on where the metal sits

• transition metals differ by 1

• Main-group metals differ by 2

Ammonium

NH4+

Hydronium

H3O+

Hydroxide

OH^1-

Peroxide

O2²-

Cyanide

CN^1-

Nitrate

NO3^1-

Acetate

CH3COO^1-

Chlorate

ClO3^1-

Bromate

BrO3^1-

Iodate

IO3^1-

Sulfate

SO4²-

Hydrogen sulfate or Bisulfate

HSO4-

Carbonate

CO3²-

Hydrogen carbonate or Bicarbonate

HCO3-

Phosphate

PO4³-

Hydrogen phosphate

HPO4²-

Dihydrogen phosphate

H2PO4-

Permanganate

MnO4^-1

Chromate

CrO4²-

Dichromate

Cr2O7²-

Ammonia

NH3

Water

H2O

Sodium hydorxide

NAOH

Hydorgen peroxide

H2O2

Hydrocyanic acid

HCN

Nitric acid

HNO3

Acetic acid

HCH3CO2

Chloric acid

HCLO3

bromic acid

HBRO3

Iodic Acid

HIO3

Sulfuric acid

H2SO4

Carbonic acid

H2CO3

Phosphoric acid

H3PO4

Perchloric acid

HCLO4

Hydrochloric acid

HCL

Hydrobromic aicd

HBR

Hydroiodic acid

HI

Polyatomic naming rules

Per - Ate is when there’s one more than normal oxygen

— ate is the starting position

— ite is when there’s one less oxygen

hypo - ate is when there’s 2 less oxygen

Hydrates and naming rules

Ionic compounds that contain water

use prefix

prefixes for hydrates and molecules

Mono - 1

Di - 2

Tri - 3

Tetra - 4

penta - 5

hexa - 6

Hepta - 7

octa - 8

nona - 9

deca - 10

Naming alkanes and what is an alkane

• An alkane is a hydrocarbon containing only single bonds

acid naming and what is an acid

• AN acid is a substance that produces H1+ ions when dissolved in water

• Two types

  • Binary acids

    • Hydorgen and a nonmetal

    • Hydro - ic acid

  • Oxyacid

    • Hydrogen and oxyanion

    • If oxyion ends with ate - ic

    • if it ends with ite - ous