UTK CHEM122 Final Exam

Density

Mass/Volume

How many significant figures are in 50.0?

3

How many significant figures are in 0.005?

1

How many significant figures are in 0.0050?

2

How many significant figures are in 50?

1

How many significant figures are in 5.00 x 10^23?

3

Precision

How close a measurement is to another measurement

Accuracy

How close a measurement is to the true value

Kilo

10^3

Centi

10^-2

Deci

10^-1

Mili

10^-3

Micro

10^-6

Nano

10^-9

Pure substance

A substance made of only one kind of matter and having definite properties

What are examples of pure substances?

Elements and compounds

Mixtures

A combination of two or more substances that are not chemically combined

Homogeneous mixtures

A mixture that is the same throughout

What are examples of homogeneous mixtures?

Coffee, air, vinegar

Heterogeneous mixtures

A mixture that is not the same throughout

What are examples of heterogenous mixtures?

Sand, dirt, cereal

Physical change

A change of matter from one form to another without a change in chemical properties

Chemical change

A change that occurs when one or more substances change into entirely new substances with different properties

What are examples of physical change?

Cutting, melting, boiling

What are examples of chemical change?

Rusting, burning, decomposing

Protons

Positively charge particles in an atom's nucleus

Neutrons

Neutrally charge particles in an atom's nucleus

Electrons

Negatively charged particles around an atom's nucleus

Isotopes

Atoms of the same element that have different numbers of neutrons

Atomic number

The number of protons in the nucleus of an atom

Mass number

The sum of the number of neutrons and protons in an atomic nucleus

Cations

Positively charged ions

Anions

Negatively charged ions

Electromagnetic radiation

A form of energy that exhibits wavelike behavior as it travels through space

Wavelength

Horizontal distance between the crests or between the troughs of two adjacent waves

Frequency

The number of complete waves that pass a given point in a certain amount of time

Photon

Particle of light

Energy of one photon equation

E = hv

Quantum number n

Principle Quantum Number

Quantum number l

Angular Momentum Quantum Number

Quantum number ml

Magnetic Quantum Number

Quantum number ms

Electron Spin Quantum Number

Principle Quantum Number

Indicates the main energy level occupied by electrons

Angular Momentum Quantum Number

Indicates the type of orbital

Magnetic Quantum Number

Indicates the orientation of an orbital around the nucleus

Electron Spin Quantum Number

Indicates the direction of the electron spin

S orbital

Holds 2 electrons

P orbital

Holds 6 electrons

D orbital

Holds 10 electrons

F orbital

Hold 14 electrons

Valence electron in Group 1A

1

Valence electron in Group 2A

2

Valence electron in Group 3A

3

Valence electron in Group 4A

4

Valence electron in Group 5A

5

Valence electron in Group 6A

6

Valence electron in Group 7A

7

Valence electron in Group 8A

8

Charge of atoms in Group 1A

+1

Charge of atoms in Group 2A

+2

Charge of atoms in Group 3A

+3

Charge of atoms in Group 5A

-3

Charge of atoms in Group 6A

-2

Charge of atoms in Group 7A

-3

Alkalai metals

Group 1A

Alkaline Earth Metals

Group 2A

Halogens

Group 7A

Nobel Gases

Group 8A

Ammonium

NH4 1+

Nitrite

NO2 1-

Nitrate

NO3 1-

Sulfite

SO3 2-

Sulfate

SO4 2-

Hydroxide

OH 1-

Phosphate

PO4 3-

Carbonate

CO3 2-

Hypochlorite

ClO 1-

Chlorite

ClO2 1-

Chlorate

ClO3 1-

Perchlorate

ClO4 1-

Permanganate

MnO4 1-

Dichromate

Cr2O7 2-

Chromate

CrO4 2-

Peroxide

O2 2-

Metals

Left side of periodic table

Nonmetals

Right side of the periodic table

Metalloids

Elements in between metals and nonmetals

Diatomic elements

H2, N2, O2, F2, Cl2, Br2, I2

Covalent bonds

Bonds between nonmetals that share electrons

Ionic bonds

Bonds between metals and nonmetals that give or take electrons

Electronegativity

A measure of the ability of an atom in a chemical compound to attract electrons

Atomic radius

The size of an atom measured by finding the distance between the nucleus' of two atoms that are bonded together

Ionization energy

The amount of energy required to remove an electron from an atom

Electron affinity

The measure of the attraction between an electron and the nucleus

Electronegativity trend

Increases up and to the right

Atomic radius trend

Increases down and to the left

Ionization energy trend

Increases up and to the right

Electron affinity trend

Increases to the right and up

Chemical formula

A formula that shows the elements in the compound and the true ratio of atoms

Empirical formula

A formula with the lowest whole-number ratio of elements in a compound