What I should know from gen chem 1

Density

ρ = m / V

zetta (Z)

10²¹

exa (E)

10¹⁸

peta (P)

10¹⁵

tera (T)

10¹²

giga (G)

10⁹

mega (M)

10⁶

kilo (k)

10³

hecto (h)

10²

deka (da)

10¹

deci (d)

10⁻¹

centi (c)

10⁻²

milli (m)

10⁻³

micro (µ)

10⁻⁶

nano (n)

10⁻⁹

pico (p)

10⁻¹²

femto (f)

10⁻¹⁵

atto (a)

10⁻¹⁸

group

Vertical column; elements share similar valence electrons and chemical behavior

period

Horizontal row; indicates number of electron shells

Alkali metals

Group 1

Alkaline earth metals

Group 2

Transition metals

Groups 3–12

Boron group

Group 13

Carbon group

Group 14

Nitrogen group

Group 15

Chalcogens

Group 16

Halogens

Group 17

Noble gases

Group 18

Hydroxide

OH⁻

Cyanide

CN⁻

Carbonate

CO₃²⁻

Bicarbonate

HCO₃⁻

Sulfate

SO₄²⁻

Sulfite

SO₃²⁻

Nitrate

NO₃⁻

Nitrite

NO₂⁻

Phosphate

PO₄³⁻

Acetate

C₂H₃O₂⁻ or CH₃COO⁻

Ammonium

NH₄⁺

Permanganate

MnO₄⁻

Chromate

CrO₄²⁻

Dichromate

Cr₂O₇²⁻

Peroxide

O₂²⁻

Steric number (SN)

Number of electron groups around the central atom (bonded atoms + lone pairs)

Electron-pair geometry

Arrangement of all electron groups around the central atom

Molecular geometry

Arrangement of bonded atoms only

SN = 2

Linear; 180°

SN = 3

Trigonal planar; 120°

SN = 4

Tetrahedral; 109.5°

SN = 5

Trigonal bipyramidal; 90° and 120°

SN = 6

Octahedral; 90°

Bent geometry

A molecular shape where the central atom is bonded to two atoms and has one or more lone pairs

Trigonal pyramidal geometry

SN = 4 with 1 lone pair; <109.5°

Seesaw geometry

SN = 5 with 1 lone pair

T-shaped geometry

SN = 5 with 2 lone pairs

Square planar geometry

SN = 6 with 2 lone pairs; 90°

Brønsted–Lowry acid

Proton (H⁺) donor

Brønsted–Lowry base

Proton (H⁺) acceptor

Conjugate acid

Species formed when a base gains a proton

Conjugate base

Species formed when an acid loses a proton

Strong acid

Completely ionizes in water

Weak acid

Partially ionizes in water

Strong base

Completely dissociates to form OH⁻

Weak base

Partially reacts to form OH⁻

Binary acid naming

hydro + root + ic acid

Oxyacid naming

-ate → -ic acid, -ite → -ous acid

Acid-base neutralization

acid + base → salt + water

Oxidation

Loss of electrons

Reduction

Gain of electrons

Oxidized species

Species that loses electrons

Reduced species

Species that gains electrons

Oxidation number

charge assigned to an atom based on electron ownership

Molar mass

Mass of one mole of a substance in grams per mole

Reactants

Substances present before a reaction

Products

Substances formed after a reaction

Polar molecule

Has a net dipole moment

Nonpolar molecule

No net dipole moment

London dispersion forces

Weak IMF present in all molecules

Dipole-dipole forces

IMF between polar molecules

Hydrogen bonding

Strong IMF when H is bonded to N, O, or F

IMF

attraction between molecules

Net dipole moment

whether a molecule has an overall uneven electron pull

Dipole

Uneven distribution of electrons in a bond that creates partial positive and partial negative ends.