Chemistry Test One Study

Front 1

WHICH GROUP IS K IN

Back 1

ALKALI METALS

Front 2

WHICH GROUP IS AR IN

Back 2

NOBLE GASES

Front 3

WHICH GROUP IS F IN

Back 3

HALOGENS

Front 4

WHICH GROUP IS BE IN

Back 4

ALKALI EARTH METALS

Front 5

WHICH GROUP IS LI IN

Back 5

ALKALI METALS

Front 6

WHAT GROUP IS MG IN

Back 6

ALKALI EARTH METALS

Front 7

WHAT GROUP IS CL IN

Back 7

HALOGENS

Front 8

WHAT GROUP IS HE IN

Back 8

NOBLE GASES

Front 9

WHAT GROUP IS BR IN

Back 9

HALGENS

Front 10

WHAT GROUP IS CA IN

Back 10

ALKALI EARTH METALS

Front 11

WHAT GROUP IS H IN

Back 11

ALKALI METALS

Front 12

WHAT GROUP IS NA IN

Back 12

ALKALI METALS

Front 13

WHAT GROUP IS RB IN

Back 13

ALKALI METALS

Front 14

WHAT GROUP IS CS IN

Back 14

ALKALI METALS

Front 15

WHAT GROUP IS FR IN

Back 15

ALKALI METALS

Front 16

WHAT GROUP IS SR IN

Back 16

ALKALI EARTH METALS

Front 17

WHAT GROUP IS BA IN

Back 17

ALKALI EARTH METALS

Front 18

WHAT GROUP IS RA IN

Back 18

ALALI EARTH METALS

Front 19

WHAT GROUP IS BR I

Back 19

HALOGENS

Front 20

WHAT GROUP IS AT IN

Back 20

HALOGENS

Front 21

WHAT GROUP IS HE IN

Back 21

NOBLE GASES

Front 22

WHAT GROUP IS AR IN

Back 22

NOBLE GASES

Front 23

WHAT GROUP IS NE IN

Back 23

NOBLE GASES

Front 24

WHAT GROUP IS KR IN

Back 24

NOBLE GASES

Front 25

WHAT GROUP IS XE IN

Back 25

NOBLE GASES

Front 26

WHAT GROUP IS RN IN

Back 26

NOBLE GASES

Front 27

Atoms are made up of:

Back 27

Protons
Neutrons
Electrons

Front 28

Cation

Back 28

There are more protons in the atom because we lost ELECTRONS

-Has a positive charge because there are more protons in the atom

Front 29

• Anion
o

Back 29

Has a negative charge because more electrons in the atom than protons

We gained ELECTRONS, the amount of protons stays the same

Front 30

o Alkali Metals

Back 30

 First column on the left
 VERY REACTIVE
 Shiny
 Soft

Front 31

• Nonmetals

Back 31

o Nonconductor
o Mostly in upper right part of table

Front 32

o Halogens

Back 32

 Second column in from the right
 Reactive

Front 33

o Noble Gases

Back 33

 First column from the right
 Stable- NOT reactive

Front 34

 Ionic Bonding

Back 34

• Results from electrostatic attraction between cations and anions

Front 35

 Covalent Bonding

Back 35

• Atoms SHARE electrons

Front 36

What are the degrees of the below shapes.

Electron Pair Geometry

Linear
Trigonal Planer
Tetrahendral

Back 36

Linear (180 degrees)
Trigonal Planar (120 degrees)
Tetrahedral (109.5 degrees)

Front 37

What is Dipole-dipole Attraction

Back 37

MUST be POLAR to have dipole-dipole
• Polar= asymmetric
• Nonpolar= symmetric (doesn’t exist in dipole-dipole)

Front 38

London Dispersion Forces

Back 38

charged seperation of electrons
 All you need to know is that this exist in ALL MOLECULES!
 The bigger the molecule, the stronger the London Dispersion is

Front 39

Hydrogen Bonding

Back 39

Occurs between hydrogen atom bonding with nitrogen, oxygen, fluorine, and a lone pair of electrons attached to the N, O, or F
• Example: ö – H
o The oxygen is bonded to the hydrogen and has a lone pair attached to it also; all this must be present for hydrogen bonding to occur
 If a molecule has Hydrogen bonding, then it will always have all three intermolecular attractions!

Front 40

What is pH

Back 40

measure of how many hydrogen ions are floating around; a numerical measure of the acidity or basicity of a solution
o lower pH number= acid
o higher pH number= basic

Front 41

What is definition of ph

Back 41

o ph= the negative logarithm of the hydronium ion concentration of a solution….in other words… –log of H+ concentration

Front 42

Definitions:

Acid

Base

Salt

Back 42

o Acid compound that dissolves in water to produce hydrogen ions (H+)
o Basedissolves in water to produce hydroxide ions (OH-)
o Salt an ionic compound consisting of a cation base and an anion acid

Front 43

Oxidation rules

Back 43

 Monoatomic ions is the charge on the ion (Na+)
 Compound F is ALWAYS has an oxidation number of -1
 Oxygen has an oxidation number of -2 UNLESS it is bonded to F then it has an oxidation number of +2
 H has oxidation number of +1
 Halogens are always -1 unless bounded to F or oxygen then they’re +1
 The sum of all the oxidation numbers has to equal the charge on the compound

Front 44

What is a Oxidation


Back 44

 Gain of oxygen
 Loss of hydrogen
 Loss of an electron

Front 45

What is a reduction

Back 45

Loss of oxygen
 Gain of hydrogen
 Gain of electron

Front 46

What are kinetics

Back 46

Study of the rates (speed) of chemical reactions

Front 47

What is rate

Back 47

The change of concentration per unit time.

Pyr concentration/pyr time=rate

Front 48

What is a Catalyst

Back 48

used in chemical reaction and increases reaction rate but not consumed in the reaction; helps particles get in proper orientation

Front 49

What are Enzymes

Back 49

 large molecules which catalyze specific biochemical reactions

Front 50

• Le Chatelier Principle (definite test question)
o

Back 50

If you add more to one side of equation, then the other side will get some too as long as the equation is at equilibrium (double arrows pointing both ways in a reaction)

Front 51

What are Acids

Back 51

Sour taste
 Gives H+ ions
 Reacts with metals to give hydrogen
 Examples: vinegar, tomatoes, citrus fruit, aspirin
o

Front 52

What are Bases

Back 52

Bitter taste
 Provides OH-
 Slippery feeling
 Examples: ammonia, soap, baking soda, detergents

Front 53

What is a precipitation reaction

Back 53

Involves the formation of an insoluble product or products from the reaction of suluble reactants.

Front 54

HCL

Back 54

Hydrochloric Acid

Front 55

HNO3

Back 55

Nitric Acid

Front 56

H2SO4

Back 56

Sulfuric Acid

Front 57

HI

Back 57

Hydro Ionic Acid

Front 58

HBr

Back 58

Hydrobromic Acid

Front 59

HCLO4

Back 59

PROCHLORIC ACID

Front 60

Name the Alkali Metal Oxides

Back 60

LIOH
KOH
NaOH
RbOH
CsOH
FrOH

Front 61

Name the Alkali Earth Metals

Back 61

Be(OH)2
Mg(OH)2
Ca(OH)2
Sr(OH)2
Ba(OH)2
Ra(OH)2

Front 62

Neutralization Reaction

Back 62

Is the reaction of an acid with a base to form a salt and water.

Front 63

Acid

Back 63

a compound that completely dissolves in water to produce hydrogen ions.

Front 64

Base

Back 64

Dissolves in water to produce hydroxide ions. It is usually a soluble metal hydroxide.

Front 65

Salt

Back 65

an ionic compound consisting of the cation of a base, and the anion of an acid.

Front 66

NH4OH-

Back 66

Ammonium Hydroxide

Front 67

Net Ionic Equation

Back 67

Shows only those species in the solution that actually undergo a chemical change.

Front 68

what is a hydronium ion

Back 68

A hydrated proton H30+

HCL + H2O -------------H3O+ CL-

Front 69

Acid Base Indicator

Back 69

Substances that change color with changes in acidity or basicity of a solution.

Front 70

Strong acids and bases _______ in water. Weak Acids and Bases establish _______in water

Back 70

Dissociate

Equilibrium

Front 71

Bracketing a species indicates
[H3O+]; [OH-]

Back 71

CONCENTRATION

Front 72

IF THE PH = 7.0 THEN THE SOLUTION IS

Back 72

NEUTRAL

[H3O+] = [OH-]

Front 73

WHAT IS A BUFFER

Back 73

A BUFFER IS A SOLUTION OF A WEAK ACID OR BASE AND ITS CONJUGATE PARTNER.