CH.1-3 Knowledge Check Study Set

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kilo (k)

10^3 = 1000

hecto (h)

10^2 = 100

deka (da)

10^1 = 10

base unit

10^0 = 1

deci (d)

10^-1 = 0.1

centi (c)

10^-2 = 0.01

milli (m)

10^-3 = 0.001

micro (μ)

10^-6 = 0.000001

nano (n)

10^-9 = 0.000000001

pico (p)

10^-12 = 0.000000000001

1 kilometer

1000 meters

1 meter

100 centimeters

1 centimeter

10 millimeters

1 kilogram

1000 grams

1 gram

1000 milligrams

1 liter

1000 milliliters

1 milliliter

1 cubic centimeter (1 cm³)

1 liter

1000 cubic centimeters (1000 cm³)

Kelvin from Celsius

K = °C + 273.15

Celsius from Kelvin

°C = K − 273.15

Fahrenheit from Celsius

°F = (9/5 × °C) + 32

Celsius from Fahrenheit

°C = (°F − 32) × 5/9

Water freezes

0°C = 273.15 K = 32°F

Water boils

100°C = 373.15 K = 212°F

SI unit for length

meter (m)

SI unit for mass

kilogram (kg)

SI unit for time

second (s)

SI unit for temperature

kelvin (K)

SI unit for amount of substance

mole (mol)

Density formula

d = m/V

Mass formula

m = dV

Volume formula

V = m/d

Common density units

g/mL or g/cm³

Atomic number

Number of protons

Mass number

Protons + neutrons

Neutrons

Mass number − atomic number

Electrons in a neutral atom

Equal to the number of protons

Fluoride

F⁻

Chloride

Cl⁻

Bromide

Br⁻

Iodide

I⁻

Oxide

O²⁻

Sulfide

S²⁻

Nitride

N³⁻

Phosphide

P³⁻

Ammonium

NH₄⁺

Hydroxide

OH⁻

Nitrate

NO₃⁻

Nitrite

NO₂⁻

Carbonate

CO₃²⁻

Hydrogen carbonate (bicarbonate)

HCO₃⁻

Sulfate

SO₄²⁻

Sulfite

SO₃²⁻

Phosphate

PO₄³⁻

Acetate

C₂H₃O₂⁻ (CH₃COO⁻)

Cyanide

CN⁻

Permanganate

MnO₄⁻

Chromate

CrO₄²⁻

Dichromate

Cr₂O₇²⁻

mono

1

di

2

tri

3

tetra

4

penta

5

hexa

6

hepta

7

octa

8

nona

9

deca

10

Ionic compound naming

Metal first + nonmetal ending in "-ide"

Transition metal naming

Use Roman numerals to indicate charge

Covalent compound naming

Use Greek prefixes

CO

Carbon monoxide

CO₂

Carbon dioxide

N₂O₅

Dinitrogen pentoxide

Diatomic elements

H₂ N₂ O₂ F₂ Cl₂ Br₂ I₂

Mnemonic for diatomic elements

Have No Fear Of Ice Cold Beer

Element

A pure substance made of one type of atom

Compound

A pure substance made of two or more elements chemically combined

Ionic bond

Occurs between a metal and nonmetal by electron transfer

Covalent bond

Occurs between nonmetals by sharing electrons

Empirical formula

Simplest whole-number ratio of atoms

Molecular formula

Actual number of each type of atom in a molecule

Structural formula

Shows how atoms are connected by bonds

Law of Conservation of Mass

Matter is neither created nor destroyed in a chemical reaction

Law of Definite Proportions

A compound always contains the same elements in the same mass ratio

Law of Multiple Proportions

Elements can combine in different whole-number ratios to form different compounds

Dalton's Atomic Theory

Atoms are indivisible, atoms of an element are identical, compounds form by whole-number ratios, atoms rearrange in reactions

Cathode rays

Streams of negatively charged electrons

J. J. Thomson

Discovered the electron using the cathode ray tube

Robert Millikan

Measured the charge of the electron using the oil drop experiment

Ernest Rutherford

Discovered the nucleus with the gold foil experiment

Plum pudding model

Electrons embedded in a positively charged sphere

Nuclear theory of the atom

Positive charge and most mass are concentrated in the nucleus

Alpha particle (α)

+2 charge, relatively heavy

Beta particle (β)

High-speed electron

Gamma ray (γ)

High-energy electromagnetic radiation