(NOT MINE) TTU CHEM 1307 Exam I

Texas Tech University, Prof. Casadonte, taken from Quizlet

Base Unit of Length

Meter (m)

Basic Unit of Mass

Kilogram (kg)

Basic Unit of Time

Second (s)

Basic Unit of Temperature

Kelvin (K)

Basic Unit of Amount of Substance

Mole (mol)

Basic Unit of Electric Current

Ampere (A)

Basic Unit of Luminous Intensity

Candela (cd)

Celsius=

F-32/1.8

Kelvin=

Celsius+273.15

Derived Unit

A combination of units

Density

Mass/Volume

Accuracy

Refers to how close the measures value is to the actual value

Precision

Refers to how close a measurements are to one another or how reproducible they are.

1 inch

2.54 centimeters

Conversion Factor

A fractional quantity with the units we are converting from on top and the units are converting to on top.

Law of Conservation of Mass

In a chemical reaction, matter is neither created nor destroyed

Law of Definite Proportions

All samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements

Law of Multiple Proportions

When two elements (call them A and B) form two different compounds, the masses of element B that combine with 1g of element A can be expressed as a ratio of small whole numbers

John Dalton Atomic Theory of 1808

1. Each element is composed of tiny, indestructible particles called atoms
2. all atoms of a given element have the same mass and other properties that distinguish them from the atoms of other elements
3. Atoms combine in simple, whole number rations to form compounds
4. Atoms of one element cannot change into atoms of another element. In a chemical reaction, atoms only change the way that they are bound together with other atoms

Ions

Results from either a gain or loss of electron

+ charge

Losses electrons

- charge

Gains electrons

Avogadros Number

6.022X10^23

a
X
z

a- mass number
z- atomic number
X- chemical symbol

z- number of protons
a- number of protons +number of neutrons

Metalloids

B, Si, Ge, As, Sb, Te, and At

Ions w/ predictable charges

H+
Li+
Na+
K+
Rb+
Cs+
Mg^2+
Ca^2+
Sr^2+
Ba^2+
Al^3+
N^3-
O^2-
S^2-
Se^2-
Te^2-
H-
F-
Cl-
Br-
I-

Alkaline

Group 1A-- + charge
(losses 1 electron)

Alkaline Earth Metals

Group 2A-- +2 charge
(losses 2 electron)

Halogens

Group 7A-- -charge
(gains 1 electron)

Noble Gases

Group 8A-
He
Ne
Ar
Kr
Xe
Rn

Covalent Bonds

Occur between two or more nonmetals

Cation

A positively charged ion

Anion

A negatively charged ion

Ionic Bonds

A metal and a nonmetal combine

Ways to Represent Compounds

Molecular Formula
Empirical Formula
Ball-and-stick Model
Space-filling Model
Structural Formula

Atomic Elements

Elements that exist in nature with single atoms as their base units, most elements fall into this category.

Molecular Elements

Do not normally exist in nature with single atoms as their basic units; instead they exist as molecules-- two or more atoms bonded together

Molecular Compounds

Composed of two or more covalently bonded nonmetals

Ionic Compounds

Composed of cations (usually a metal) and anions (usually one or more nonmetals)

Qualitative

Noting or describing how a process hapoens

Quantitative

Measuring or quantifying something about the process

Antoine Lavoisier

(1743-1794) first chemist to use quantitative method, he studied combustion

Observations

Referred to as data formed into a hypothesis

Hypothesis

Tentative interpretation, further experiments to test

Scientific Law

-Lead to by a series of similar observations
-A brief statement that summaries past observations and predicts future ones

Theory

Well established hypothesis may form basis for a scientific theory.
Definition: explanation of the general causes of certain phenomena, with considerable evidence or faces to support it

Homogenous Mixture

Mixture of same compositions

Physical Change

Alter only the state or appearance

Heterogenous Mixture

Mixture of different compositions

Chemical Change

Alter the composition

Giga

Symbol: G
Multiplier: 10^9

Mega

Symbol: M
Multiplier: 10^6

Kilo

Symbol: k
Multiplier: 10^3

Deci

Symbol: d
Multiplier: 10^-1

Milli

Symbol: m
Multiplier: 10^-3

Micro

Symbol: u
Multiplier: 10^-6

Nano

Symbol: n
Multiplier: 10^-9

Pico

Symbol: p
Multiplier: 10^-12

Intensive Property

Independent of the amount of substance; ex: boiling or melting point

Extensive Property

Dependent of the amount of substance; ex: mass and volume

Decanting

Carefully pulling off water
Separating a solid and a liquid

Distillation

Process in which the mixture is heated to boil off the more volatile (easily vaporizable) liquid

Filtration

The mixture is poured through filter paper in a funnel

Fractional Subscript- Multiply by This

.02 - 5
.25- 4
.33- 3
.40- 5
.50- 2
.66- 3
.75- 4
.80- 5

Acetate

C2H3O2^-

Carbonate

CO3^2-

Hydrogen Carbonate (bicarbonate)

HCO3^-

Hydroxide

OH^-

Nitrite

NO2^-

Nitrate

NO3^-

Chromate

CrO4^2-

Dichromate

Cr2O7^2-

Phosphate

PO4^3-

Hydrogen Phosphate

HPO4^-

Dihydrogen Phosphate

H2PO4^-

Ammonium

NH4^+

Hypochlorite

CIO^-

Chlorite

CIO2^-

Chlorate

CIO3^-

Perchlorate

CIO4^-

Permanganate

MnO4^-

Sulfite

SO3^2-

Hydrogen Sulfite

HSO3^-

Sulfate

SO4^2-

Hydrogen Sulfate

HSO4^-

Cyanide

CN^-

Peroxide

O2^2-

Hemi

1/2

Mono

1

Di

2

Tri

3

Tetra

4

Penta

5

Hexa

6

Hepta

7

Octa

8

Nona

9

Deca

10

Binary Acids

-Composed of hydrogen and a nonmetal
-Hydro-base name of nonmetal-acid
-ends in -ic

Oxyacids

-Contain hydrogen and an oxyanion (an anion containing a nonmetal and oxygen)
-base name of oxyanion+acid

-ate--> ic
-ite--> ous