Test 1

Law

a concise statement or mathematical equation about a fundamental relationship or regularity of nature

Hypothesis

a tentative explanation of some regularity of nature

experiment

observation of natural phenomena carried out in a controlled manner so that the results can be duplicated and rational conclusions obtained

Theory

a tested explanation of a basic natural phenomenon

Law of conservation of mass

the total mass remains constant during a chemical change

Measurement

the comparison of a physical quantity to be measured with a unit of measurement

Precision

the closeness of the set of values obtained from repeated measurement of the same quantity

accuracy

the closeness of a single measurement to its true value

Significant figures

those digits that include all certain digits plus a final one having some uncertainty

All _____ digits are significant

All nonzero digits are significant

Sig Figs:
When multiplying or dividing...

When multiplying or dividing, give as many sig fig as the least

Sig Figs:
When adding or subtracting...

When adding or subtracting, give as many decimals as the least

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)

SI unit for electric current

Ampere (A)

Derived Units

Constitutes a combination of fundamental units
e.g: Volume, Speed, Density

Ammonium ion

NH4+

Mercury(I) Ion

Hg2 2+

hydronium ion

H3O+

Phosphonium Ion

PH4+

Azide Ion

N3-

Acetate ion

C2H3O2- or CH3COO-

Oxalate ion

C2O4 2-

Nitrate ion

NO3-

Nitrite Ion

NO2-

Hydroxide Ion

OH-

Hydrogen Carbonate Ion or Bicarbonate

HCO3-

Hydrogen Sulfate Ion

HSO4-

Cyanide Ion

CN-

Permanganate Ion

MnO4-

Perchlorate ion

ClO4-

Chlorate ion

ClO3-

Chlorite ion

ClO2-

Hypochlorite ion

ClO-

Carbonate ion

CO3 2-

Sulfate ion

SO4 2-

Sulfite ion

SO3 2-

Hydrogen Sulfite Ion or Bisulfite Ion

HSO3-

Hydrogen Sulfate Ion or Bisulfate Ion

HSO4-

Borate ion

BO3 3-

Iodate ion

IO3-

Bromate ion

BrO3-

Chromate ion

CrO4 2-

Dichromate ion

Cr2O7 2-

Peroxide Ion

O2 2-

Phosphate ion

PO4 3-

Monohydrogen phosphate ion

HPO4 2-

Dihydrogen phosphate ion

H2PO4-

Cyanide ion

CN-

Cyanate ion

OCN-

Thiocyanate ion

SCN-

In inorganic substances cations:

have the same name as the metal they originate from
(put roman numeral after middle metals)

In inorganic substances monatomic anions:

end in "ide"

In inorganic substances oxoanion:

Polyatomic ions usually end in "ate" or "ite"

When adding hydrogen to an oxoanion:

Use hydrogen or dihydrogen as a prefix

In ionic compounds ___ is named 1st followed by __

Cation is named 1st followed by anion

For acids with an "ide" anion

prefix is hydro
suffix is "ic acid"

Acids with "ate" polyatomic ion

change "ate" to "ic" followed by acid

Acids with "ite" polyatomic ion

change "ite" to "ous acid:

Binary molecular compounds (made of two nonmetals)

The less electronegative element is named 1st and unchanged
The more electronegative has an ide ending and a prefix added

Mono

1

di

2

tri

3

tetra

4

penta

5

1 amu = _ Dalton (Da)

1 amu = 1 Dalton (Da)

1 atomic mass unit equals __ a __ atom

1 atomic mass unit equals 1/12th a Carbon-12 atom

Matter

Whatever occupies space and can be perceived by our senses

Mass

The quantity of matter in a material

Classification

Its physical state: solid, liquid, or gas
Its chemical constitution: element, compound, or mixture

Intensive Property

a property that is independent of the amount of substance present

Extensive Property

a property that varies with the quantity of the substance present

Physical Property

A characteristic that can be observed for a material without changing its chemical identity

Chemical Property

A characteristic of a material involving its chemical change

Physical Change

A change in form of matter but not its chemical identity
Mostly reversible
No new compounds are found

Chemical Change

New compounds are formed
In many cases the process is nonreversible
Chemical reactions

Types of matter

Pure substance
Mixture

Pure Substance

Same physical and chemical properties throughout
Can't be separated into simpler substances by a physical process

Mixture

Combination of 2 or more pure substances
Can be separated by physical processes

3 ways to separate mixtures

Distillation
Filtration
Chromatography

Law of Definite Proportions

a pure compound, regardless of its source always contains constant proportions of the elements by mass

Electrons

Negatively charged particles

Protons

Positively charged particles

Neutrons

uncharged particles

Atomic number

Number of protons in nucleus

Mass number

number of protons plus number of neutrons

nuclide

atom with a definite atomic number and mass number

Isotopes

Atoms whose nuclei have the same number of protons but different number of neutrons

Average Atomic Mass

Weighted average of masses of all isotopes of a element

Natural Abundance

Proportion of a particular isotope; usually expressed as a percent relative to all the isotopes for that element in a natural sample

Period (periodic table)

Elements in 1 row

Group (periodic table)

Elements in 1 column

Mendeleev's discovery

If elements were arranged in order of atomic number, they could be placed in horizontal rows such that the elements in the vertical columns had similar properties.

Bonds

Ionic Bond
Covalent Bond

Molecule

A definite group of atoms that are chemically bonded together

Organic Compounds

Carbon combined with other elements, such as hydrogen, oxygen, and nitrogen

Inorganic Compounds

composed of elements other than carbon