Final exam study terms

Chemistry terms from all 3 trimesters

alkali metals

most reactive metals; group 1A on the periodic table; all have 1 valence electron

alkaline earth metals

group 2A on the periodic table; all have 2 valence electrons

transition metals

Family of elements in the middle of the periodic table; elements like iron and copper are in this group.

noble gases

group 8A on the periodic table; also known as the "inert" gases, NON-reactive, have full outer shell of electrons (He-full w/2 electrons, Ne-Rn full 8)

halogens

most reactive non-metals, group 7A on periodic table; all have 7 valence electrons

group/family

column on the periodic table, share similar physical and chemical properties & same valence electrons

period

row on the periodic table; shows an atoms occupied energy levels

ionization energy

the energy required to remove a valence electron and form a positive ion.

trend in atomic size

increases down a group, decreases across a period (left to right)

trend in ionization energy

decreases down a group (easier to remove electrons as you go down), increases across a period from left to right (harder to remove electrons as you move right).

valence electron

The electrons that are farthest away from the nucleus--in the outermost shell and are involved in chemical reactions. These electrons mainly determine the chemical properties of an element

Cation

When an atom loses an electron (+ ion) atomic radius will decrease

Anion

When an atom gains an electron (- ion) atomic radius will increase

Metallic elements

Elements that are usually solids at room temperature, exhibit high electrical and heat conductivity, and appear lustrous; tend to lose electrons in reactions.

Nonmetals

Elements that are poor conductors of heat and electric current; tend to gain electrons in reactions.

+1

Charge of group 1 ions

+2

Charge of group 2 ions

-2

Charge of group 6 ions

-1

Charge of group 7 ions

-3

Charge of group 5 ions

Atomic number

the number of protons in the nucleus of an atom

Atomic symbol

one or two letter chemical shorthand for each element

Mass number

The total number of protons and neutrons in the nucleus of an atom

Proton

Positively charged particle in the nucleus of an atom.

Neutron

Neutrally charged particle in the nucleus of an atom

Electron

Negatively charged particle; located outside the atomic nucleus. Determines the chemical properties of an element.

Nucleus

Center of an atom, very small portion of the atom where all of the mass and + charge is located

Isotopes

Atoms of the same element that have different numbers of neutrons

Isotope Notation

common notation used to specify the specific version of an atom; ie C-14 or 14/6 C

Energy level

Appear as rings around the nucleus representing specific distances which electrons of the same energy are be found

Subatomic particle

Found within the atom, mainly protons, neutrons, and electrons.

Ion

A charged atom resulting from the gain or loss of electrons

Precipitate reaction

a double replacement reaction where two aqueous salts react producing an insoluble solid.

average kinetic energy

The measure of energy of the particles in substance = temperature.

Reactant

a starting substance in a chemical reaction

Product

A substance produced in a chemical reaction (new substance created)

Factors affecting Solubility

nature of solute and solvent, temperature, pressure, and surface area

Chemical change

A change in matter that produces one or more new substances

Physical change

A change in a substance that does not involve a change in the identity of the substance

chemical property

Describes a substances ability to react with other substances. Examples: Lithium reacts water, wood burns (reacting with oxygen) or Noble gasses will not react at all.

physical property

a characteristic that can be observed or measured without changing the identity of the substance; examples include include density, color, hardness, melting and boiling points, and electrical conductivity

Solid

Definite shape and volume; low particle spacing and energy.

Liquid

no definite shape but has a definite volume; medium particle spacing & energy.

Gas

no definite shape or volume

Plasma

highest energy state of matter where electrons temporarily leave the atom

Conservation of mass

mass cannot be created or destroyed

Molar mass

The mass of one mole of a substance in grams; mass number on the periodic table

Octet rule

States that atoms lose, gain or share electrons in order to acquire a full set of eight valence electrons

Celcius

Metric temperature scale on which water freezes at 0 degrees and boils at 100 degrees

Kelvin

Unit for temperature based on absolute zero = 0

Molarity

the number of moles of solute per liter of solution (m/L)

Mole calculation

Moles = grams/molecular mass

Density

mass/volume

Dilution

M1V1=M2V2

Adding water to a solution in order to decrease the concentration

Solute

A substance that is dissolved in a solution (minor component of mixture)

Solvent

A liquid substance capable of dissolving other substances (major component of mixture)

homogeneous mixture

A mixture in which substances are evenly distributed throughout the mixture; ie pills containing different chemical compounds

heterogeneous mixture

A mixture in which different materials can be distinguished easily; uneven distribution

gas temperature

Measure of average kinetic energy of gas particles.

Atomic radius

size of an atom; increase when electrons are gained or decrease when electrons are lost. Atoms lower on the PT are larger.

'stair case'

metalloids, separates metals (left) from non metals (upper right) on the periodic table

PV=nRT

ideal gas law equation

6.02x10²³

1 mole; aka Avogadro's number

Balanced chemical equation

chemical equation with the same number of atoms of each element on both sides of the equation. To balanced an unbalanced equation you add correct coefficients.

symbols for states of matter

(s) solid, (l) liquid, (g) gas, (aq) aqueous or dissolved in water; ie H2O(s) indicates ice not water

the octet rule

The concept that states that atoms tend to gain, lose, or share valence electrons so that they can have 8 electrons in their outer shell

'ide'

In an ionic compound the non metal ends with _

SO4

Sulfate -2

nonpolar covalent bond

equal sharing of electrons

chemical analysis

a process used to determine the composition of a substance; can be used to verify if a reaction produces a new substance

Avogadro's number

One mole = 6.02 x 10^23

polar covalent bond

unequal sharing of electrons

pH

Acid/Base scale from 0-14 based on the concentration of hydrogen ions in a solution.

Direct

Relationship where an increase in one variable results in an increase in the other variable (more is more)

Inverse

Relationship where an increase in one variable results in a

Kelvin

Temperature scale that is based on absolute zero; gas law calculations need to be in this scale.