Finals Review

Front 1

Solvent

Back 1

The component of a solution that is present in the greatest amount.

Hint 1

It is the substance in which the solute is dissolved.

Front 2

Solute

Back 2

Substance that is dissolved in a solution.

Front 3

Oxyacid

Back 3

Any acid containing oxygen.

Front 4

Acid

Back 4

Hydrogen ions in a water solution that combined with bases.

Front 5

Oxyanion

Back 5

Onion containing one or more oxygen atoms bonded to another element.

Front 6

Anion

Back 6

A negatively charged ion

Front 7

Cation

Back 7

A positively charged ion

Front 8

Covalent bond

Back 8

A chemical bond that involves sharing of pair of electrons between atoms in a molecule

Front 9

Ionic bond

Back 9

A chemical bond between oppositely charged ions

Front 10

Chemical Bond

Back 10

Electrostatic force linking atoms

Front 11

reactant

Back 11

Substances that react in a chemical change

Front 12

Product

Back 12

Substances that are formed by the chemical change

Front 13

Subatomic particles

Back 13

Protons, electrons, neutrons

Front 14

Isotope

Back 14

Atoms of the same element that have different masses

Front 15

Electromagnetic radiation

Back 15

The form of energy that exhibits wavelike Behavior as it travels through space

Front 16

Frequency

Back 16

The number of waves that pass a given point in a specific time

Front 17

Wavelength

Back 17

Distance between corresponding points on adjacent waves

Front 18

Photoelectric effect

Back 18

Refers to the emission of electrons from a metal when light shines on the metal

Front 19

Quantum

Back 19

The minimum quantity of energy that can be lost or gained by an atom

Front 20

Heisenberg's uncertainty principle

Back 20

States that it is impossible to determine simultaneously both position and velocity of an electron or any other particle

Front 21

Aufbau principle

Back 21

An electron occupies the lowest energy orbital that can receive it

Front 22

Hund's Rule

Back 22

Orbital's of equal energy are eight occupied by one electron before any orbital is occupied by say electron and all electrons are singularly occupy orbitals must have the same spin state

Front 23

Pauli Exclusion Principle

Back 23

No two electrons in the same atom can have the same set of four quantum numbers

Front 24

Boyle's Law

Back 24

States that the volume of a fixed mass of gas varies inversely with the pressure at a constant temperature

Front 25

Solution

Back 25

A homogeneous mixture of two or more substances in a single phase

Front 26

Electronegativity

Back 26

Attraction of an elemental particle to its valence electron measured on a number scale

Front 27

Lewis diagram / Electron Dot Structure

Back 27

A diagram system that represents covalent bonds and their shared electrons using lines and unshared the valence electrons with

Front 28

Overall charge of ionic compound

Back 28

Neutral

Front 29

Ionic bonds occur between?

Back 29

Metal and nonmetal

Front 30

Molecule

Back 30

The smallest particle of an element or compound capable of a stable, independent existence.

Front 31

VSEPR Model

Back 31

Assumes that electron pairs are arranged around the central element of a molecule or polyatomic ion so that there is maximum separation and minimum repulsion among regions of high electron density.

Front 32

Polar Covalent Image

Back 32

a type of chemical bond where a pair of electrons is unequally shared between two atoms.

Front 33

Structure formula

Back 33

a formula that shows the arrangement of atoms in the molecule of a compound.

Front 34

Carbonic acid

Back 34

H2C

Front 35

Carbon dioxide

Back 35

C2D

Front 36

Carbon monoxide

Back 36

CO

Front 37

Ammonia

Back 37

NH3

Front 38

Spectator ion

Back 38

Ions in a solution that do not participate in a chemical reaction.

Front 39

Net ionic equation

Back 39

Equation that results from canceling spectator ions and eliminating brackets from a total ionic equation.

Front 40

Chemical equation

Back 40

Description of a chemical reaction by placing the formulas of the reactants on the left and the formulas of products on the right of an arrow.

Front 41

Aqueous solution

Back 41

Refers to a solution with water as solvent.

Front 42

Single replacement

Back 42

a type of chemical reaction where an element reacts with a compound and takes the place of another element in that compound.

Front 43

Double replacement

Back 43

a type of chemical reaction where two compounds react, and the positive ions (cation) and the negative ions (anion) of the two reactants switch places, forming two new compounds or products

Front 44

Synthesis

Back 44

a type of reaction in which multiple reactants combine to form a single product.

Front 45

Decomposition

Back 45

analysis or breakdown is the separation of a chemical compound into elements or simpler compounds.

Front 46

Chemical reaction

Back 46

I

Front 47

Precipitate

Back 47

An insoluble solid formed by mixing in solution the constituent ions of a slightly soluble solution.

Front 48

Aufbau principle

Back 48

Means electrons are added to orbitals as protons are added to an atom

Front 49

Valence electrons

Back 49

an electron that is associated with an atom, and that can participate in the formation of a chemical bond

Front 50

Atomic orbital

Back 50

Region or volume in space in which the probability of finding electrons is highest.

Front 51

Noble gas

Back 51

any of the gaseous elements helium, neon, argon, krypton, xenon, and radon, occupying Group 0 (18) of the periodic table.

Front 52

Quantum mechanical model of an atom

Back 52

a model that explains how electrons exist in atoms and how those electrons determine the chemical and physical properties of elements.

Front 53

Schrödinger's wave equation

Back 53

an equation that describes thewave nature of elementary particles and is fundamental to the description of the properties of all matter.

Front 54

Photo effect

Back 54

the effect of high-energy radiation (as gamma rays) on an atomic nucleus; especially : photodisintegration.

Front 55

Ground state

Back 55

Lowest energy state or most stable state of an atom, molecule or ion.

Front 56

Electron configuration

Back 56

Specific distribution of electrons in atomic orbitals of atoms or ions.

Front 57

Heisenberg uncertainty principle

Back 57

That it is impossible to measure two properties of a quantum object, such as its position and momentum (or energy and time), simultaneously with infinite precision.

Front 58

Double bond

Back 58

Covalent bond resulting from the sharing of four electrons (two pairs) between two atoms.

Front 59

Aufbau principle

Back 59

Outlines the rules used to determine how electrons organize into shells and subshells around the atomic nucleus

Front 60

Precipitate

Back 60

A solid that separates from solution.

Front 61

Single Bond

Back 61

Covalent bond resulting from the sharing of two electrons (one pair) between two atoms.

Front 62

Formula Unit

Back 62

The smallest repeating unit of a substance. The molecule for nonionic substances

Front 63

Metallic Bond

Back 63

The smallest repeating unit of a substance. The molecule for nonionic substances

Front 64

Structure Formula

Back 64

Depicts the bonding of atoms in a molecule.

Front 65

Single Replacement Formula

Back 65

Front 66

Double Replacement Formula

Back 66

Front 67

Synthesis Formula

Back 67

Front 68

Decomposition Formula

Back 68

Front 69

Synthesis Reaction

Back 69

release energy in the form of heat and light, so they are exothermic.

Front 70

Noble Gases

Back 70

They were long believed to be totally unreactive but compounds of xenon, krypton, and radon are now known.