Chem 101 OLI Torus Units 2 - 5

Common Conversions, SI Prefixes, and Compounds, and more

cm to inch

2.54cm = 1in

meters to yards

1 m = 1.0936 yd

kilometer to mile

1 km = 0.6213 mi

miles to meters

1 mi = 1609.3 m

liter to quarts

1 L = 1.0567 qt

quarts to liters

1 qt = 0.94635 L

gallons to liters

1 gal = 3.7854 L

fluid oz to milliliters

1 fl oz* = 29.5735 mL

kilogram to pounds

1 kg = 2.2046 lb

pound to grams

1 lb = 453.59 g

ounce to grams

1 oz* = 28.349 g

femto (f)

10 ^ -15

pico (p)

10 ^ -12

nano (n)

10 ^ -9

micro (μ)

10 ^ -6

milli (m)

10 ^ -3

centi (c)

10 ^ -2

deci (d)

10 ^ -1

kilo (k)

10 ^ 3

mega (M)

10 ^ 6

giga (G)

10 ^ 9

tera (T)

10 ^ 12

cm ^ 3 to mL

1 cm ^ 3 = 1 mL

kelvin to celcius

T(K) = T(C) + 273.15

celcius to kelvin

T(C) = T(K) - 273.15

Celcius to fahrenheit

(9/5) * T(C) + 32

fahrenheit to celcius

(5/9) * (T(F) - 32)

liter to decimeter ^ 3

1 L = 1 dm ^ 3

density equation

d = m/v

sig fig conversions

answer adopts smallest sig fig

sig fig addition/subtraction

round by decimal points, but keep the extra numbers

sig fig multiplication/division

round by smallest number of sig figs

Avogadro’s Number (mol)

6.02214179 × 10^23

acids

Substances that produce H3O+ when dissolved in water.

alpha (α) particle

Positively charged particle consisting of two protons and two neutrons.

anion

A negatively charged ion.

atomic theory

The theory that all matter is composed of minute particles called atoms.

binary acid

Compound containing two different elements.

binary ionic compound

Ionic compound consisting of a monatomic cation and a monatomic anion.

cation

A positively charged ion.

constant composition

A pure substance always contains the same elements in the same proportions

coordination compounds

Substances containing one or more metal complexes.

covalent compound

Molecule formed by covalent bonds, which are chemical bonds that share rather than transfer electrons.

covalent substance

Substance whose molecules are formed by covalent bonds, which are chemical bonds that share rather than transfer electrons.

diatomic molecules

Molecules consisting of only two atoms.

electron

A negatively charged subatomic particle.

empirical formula

Formula showing the simplest whole-number ratio of atoms present in a compound.

fixed mass

The ratio of the element's masses within a molecule does not change—it is constant.

formula mass

Sum of the average masses for all atoms represented in a chemical formula; for covalent compounds, this is also the molecular mass.

hydrate

A compound containing one or more water molecules bound within its crystals.

inner transition metals

Elements in the bottom two rows. Those in the first row are also called lanthanides, and those in the second row are also called actinides.

inorganic molecular compound

A chemical compound that has no carbon–hydrogen bonds.

ion

An atom that has gained or lost electrons and therefore is electrically charged.

ionic compound

compound held together by ionic bonds.

isomers

Molecules that have identical molecular formulas but different arrangements of atoms.

isotopes

Atoms of the same element that have different masses due to different numbers of neutrons.

law of definite proportions

Also called the law of constant composition, this law states that all samples of a pure compound contain the same elements in the same proportions by mass.

law of multiple proportions

When two elements react to form more than one compound, a fixed mass of one element will react with masses of the other element in a ratio of small whole numbers.

main-group elements

Elements in groups 1, 2, and 13 through 18 (also called representative elements).

mass number

The total number of protons and neutrons in an atom, represented by A.

mass ratio

The proportion of the masses of each element within a molecule.

mass spectrometry

A method used to analyze and identify the chemical composition of a substance by separating gaseous ions according to their differing mass and charge.

molar mass

Mass in grams of 1 mole of a substance.

mole

Amount of substance containing the same number of atoms, molecules, ions, or other entities as the number of atoms in exactly 12 grams of C-12.

molecular formula

A representation of a molecule that uses chemical symbols to indicate the types of atoms followed by subscripts to show the actual number of atoms of each type in the molecule.

monatomic

formed from one atom

natural abundance

Natural abundance is the average amount of an isotope that naturally occurs on Earth.

neutron

Uncharged, subatomic particle located in the nucleus.

nucleus

Massive, positively charged center of an atom made up of protons and neutrons.

organic compounds

Chemical compounds that contain carbon–hydrogen or carbon–carbon bonds.

oxyacids

Compounds that contain hydrogen, oxygen, and one other element, bonded in a way that imparts acidic properties to the compound (the ability to release H+ ions when dissolved in water).

oxyanion

Polyatomic ion that contains one or more oxygen atoms.

periodic law

The properties of the elements are periodic functions of their atomic numbers.

polyatomic ion

Ion composed of more than one atom.

postulate

A hypothesis that is accepted as true for the purposes of following a particular line of reasoning.

proton

Positively charged subatomic particle located in the nucleus of the atom.

space-filling model

A representation that shows the relative sizes of the atoms of a given substance.

structural formula

A representation of a molecule that gives the same information as its molecular formula (the types and numbers of atoms in the molecule) but also shows how the atoms are connected in the molecule.

transition metals

Element in groups 3 through 12 (more strictly defined, 3–11).

c = λv

frequency(v) and wavelength(λ) relationship, c = 2.998 × 10 ^ 8 m/s

E = hv

Energy and frequency(v) relationship, h = 6.62 × 10 ^ -34 m²kg/s

E = hv = hc/λ

energy, frequency, and wavelength relationship

Particle

energy is carried by photons, each with E = hv

Planks constant

6.62 * 10 ^ -34 m²kg / s

constant c

c = 2.998 × 10 ^8 m/s

ammonium

NH4 +

peroxide

O2²-

hydroxide

OH -

acetate

C2H3O2 -

cyanide

CN -

carbonate

CO3²-

bicarbonate

HCO3 -

nitrate

NO3 -

nitrite

NO2 -

sulfate

SO4²-

hydrogen sulfate

HSO4 -

sulfite

SO3²-

hydronium

H3O +

hydrogen sulfite

HSO3 -

phosphate

PO4³-