Ap Chemistry Summer Vocabulary

Front 1

Hydronium

Back 1

H3O+

Front 2

pH

Back 2

Measures acidity of a solution. -log[H3O+]=-log[H+]

Front 3

pOH

Back 3

Measures acidity of a solution. -log[OH-]

Front 4

pH scale

Back 4

0-14

Front 5

Hydroxide

Back 5

characteristic of bases

Front 6

Acid

Back 6

Below 7 on pH scale. Begin with H.

Front 7

Base

Back 7

Above 7 on pH scale. End in OH

Front 8

Neutral

Back 8

7 on pH scale

Front 9

Arrhenius Acids/Bases

Back 9

Donate H+(acid) or HO-(base)

Front 10

Bronsted-Lowry Acid

Back 10

Proton (H+) donor

Front 11

Bronsted-Lowry Base

Back 11

Proton (H+) acceptor

Front 12

Conjugate Acid

Back 12

Formed when a base gains a H+

Front 13

Conjugate Base

Back 13

Formed when an acid donates an H+

Front 14

Monoprotic

Back 14

Acid containing one ionizable H

Front 15

Diprotic

Back 15

Acid containing 2 ionizable Hs

Front 16

Triprotic

Back 16

Acid containing 3 ionizable Hs

Front 17

Alkane

Back 17

Simplest hydrocarbon

Front 18

Nonmetal Oxides

Back 18

Binary compound of a nonmetal and oxygen.

Hint 18

SO2

Front 19

Salts

Back 19

Ionic compounds other than bases and metal oxides.

Hint 19

NaCl

Front 20

Strong Acids

Back 20

HCl, HBr, HI, HNO3, H2SO4, HClO4

Front 21

Strong Bases

Back 21

Group I and II hydroxodes

Front 22

Soluble Salts

Back 22

All salts containing the cations sodium, potassium, or ammonium. All salts containing the anions nitrate or acetate. All chlorides except silver, lead and mercury(I).

Front 23

Ions harder to reduce than water

Back 23

Metal cations from groups I and II and Al 3+

Front 24

Ions harder to oxidize than water

Back 24

F-, NO3-, SO4 2-

Front 25

Diatomic molecules

Back 25

(H, O, N, Cl, F, I, Br) When in elemental form by themselves, usually found in pairs. Ex: O2

Front 26

Electron cloud

Back 26

Space that an electron has a high probability of occupying in an atom.

Front 27

Octet rule

Back 27

Atoms are most stable when 8 electrons are in the outer energy level.

Front 28

First ionization energy

Back 28

Energy required to remove the most loosely held electron from an atom.

Front 29

Electronegatovity

Back 29

The attraction am atom has for a shared (bonding) pair of electrons.

Front 30

Transition metals

Back 30

In the "d" block of the periodic table.

Front 31

Halogens

Back 31

Most reactive nonmetals (because of 7 electrons). Found in group 7.

Front 32

Alkali metals

Back 32

Most reactive metals. Found in group 1.

Front 33

Single bond

Back 33

One pair of electrons being shared between two atoms.

Front 34

Double bond

Back 34

Two shared pairs of electrons between two atoms. Stronger and shorter than a single bond.

Front 35

Triple bond

Back 35

Three shared pairs of electrons between two atoms. Stronger and shorter than single/double bond.

Front 36

Metallic bond

Back 36

Bond between metal atoms held together by a "sea" of delocalized electrons.

Front 37

Covalent bond

Back 37

Bond between two nonmetals

Front 38

Ionic bond

Back 38

Bond when ions are attracted

Front 39

Polar

Back 39

Uneven charge. Has a more positive and more negative side. Stronger intermolecular forces between polar molecules.

Front 40

Nonpolar

Back 40

Even charge.

Front 41

Van der Waals forces

Back 41

Generally weak intermolecular forces

Front 42

London dispersion force

Back 42

Intermolecular force found in nonpolar molecules based on size of electron cloud.

Front 43

Catalyst

Back 43

Speeds up reaction

Front 44

Product

Back 44

On right side of chemical equation. End materials.

Front 45

Reactants

Back 45

On left side of chemical equation. Starting materials.

Front 46

Limiting reagent

Back 46

The reactant that is completely used up during a reaction if it goes to completion.

Front 47

Combustion reactions

Back 47

A chemical reaction where a hydrocarbon and oxygen produce carbon dioxide and water.

Front 48

Entropy

Back 48

Measure of disorder. Gases have the most. Solids have the least.

Front 49

Enthalpy

Back 49

The heat content of a system.

Front 50

Molecular compound

Back 50

Compound formed by covalent bonds.

Front 51

Valence electrons

Back 51

Outer level electrons of an element.

Front 52

Ionic compound

Back 52

Formed when a metal(+) and a nonmetal(-) combine.

Front 53

Dipole

Back 53

Intermolecular force between two polar molecules.

Front 54

Enzymes

Back 54

Catalysts found in the body

Front 55

Reversible reaction

Back 55

Reaction can proceed in both directions. Represented with double arrows.

Front 56

Spectator ions

Back 56

Ions that do not participate in the chemical reaction.

Front 57

Anode

Back 57

The electrode where oxidation occurs.

Front 58

Cathode

Back 58

The electrode where reduction occurs.

Front 59

Oxidation number

Back 59

Charge on a single atom showing how many electrons it's lost or gained.

Front 60

Redox reaction

Back 60

Reaction where electrons are transferred.

Front 61

Reduction

Back 61

Gaining electrons, oxidation number becomes more negative.

Front 62

Oxidation

Back 62

Loss of electrons, oxidation number becomes more positive.

Front 63

Alloy

Back 63

Solution made of two metals

Front 64

Standard solution

Back 64

Solution with a known concentration

Front 65

Molarity

Back 65

Moles of solute per liter of solution

Front 66

Solute

Back 66

Gets dissolved (solid)

Front 67

Solution

Back 67

Homogeneous mixture

Front 68

Mixture

Back 68

Material consisting of 2 or more substances that can be homogeneous or heterogeneous.

Front 69

Precipitate

Back 69

A solid produced by two solutions.