Chem Chapter 2

Front 1

Law of conservation of mass

Back 1

The total mass of material present after a chemical reaction is the same as the total mass present before the reaction.

Front 2

Law of multiple proportions. Dalton

Back 2

If 2 elements A & B combine to form more than one compound, the masses of B that combine with a given mass of A are in the ratio of small whole numbers.

Front 3

Dalton's atomic theory, 4 postulates

Back 3

1 - small particles called atoms form each element

2 - atoms from each element are identical, and different from atoms of a different elements

3 - atoms of an element cannot be changed into atoms of a different element and atoms cannot be created or destroyed in chemical reactions.

4 - elements can combine atoms to form compounds. A given compound always have the same relative number and type of elements.

Front 4

What did the Cathode Ray experiment help discover? When was the paper published?

Back 4

Electrons and their charge to mass ratios. 1897.

Front 5

What is electric charge of an electron? To its mass?

Back 5

-1.602x10^-19, 1.76 x 10^8 coulombs per gram

Front 6

How was the electric charge of an electron measured?

Back 6

Using Cathode rays and calculating the strength of magnets and electric forces needed to deflect the electrons.

Front 7

Approximate diameter of the nucleus

Back 7

100-500 picometers. Or 1-5 angstroms.

Front 8

The elements that normally occur as diatomic molecules.

Back 8

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

Front 9

Molecules are composed of:

Back 9

Two types or more types of atoms from different elements, generally composed of non-metals only.

Front 10

Methane formula

Back 10

CH4

Front 11

Methane formula

Back 11

CH4

Front 12

Ionic compounds are generally formed from which types of elements? What about molecular compounds?

Back 12

Combinations of metals and nonmetals.

Molecular compounds are composed of Nonmetals only. Like H2O.

Front 13

How to figure empirical formula for ionic compounds.

Back 13

Take the charges number and make it the subscript for the other element.

Front 14

How to name ionic compounds?

Back 14

Cations formed from metal atoms have the same name as the metal. If the metal can have two charges then the positive charge is indicated by a Roman numberal in parentheses following the name of the metal.

Anions: the names of monatomic anions are formed by replacing the ending of the name of the element with -ide. EX: H^-Hydride ion. O^2- oxide ion. N^3- nitride ion.

Hint 14

Cations, anions, metals with two charges, and monatomic examples.

Front 15

Which elements can have more than one charge?

Back 15

Most metals that can form two different charges are transitional metals from the middle of the periodic table (group 3B to 2B).

Front 16

Which metals can only form one charge?

Back 16

Group 1A and 2A, as well as Al^3+ and two transitional metals: Ag^+ and Zn^2+. Charges are not expressed when writing these ions. When in doubt, write the charges in Roman numberal since it is never considered wrong to do so.

Front 17

The older method of distinguishing different transitional ionic charges.

Back 17

The lesser charge: add -ous to element name. EX: ferrous ion (Fe^2+). The higher charge: -ic. EX: cupric ion (Cu^2+)

Front 18

Cations formed from nonmetal atoms have names that end in?

Back 18

-ium. Ex: NH4^+ = ammonium ion. H3O^+ = hydronium ion.

Front 19

Cations with 1+ charges

Back 19

H^+, Li^+, Na^+, K^+, Cs^+, & Ag^+.

Front 20

Ions with 2+ charges.

Back 20

Mg^2+, Ca^2+, Sr^2+, Ba^2+, Zn^2+, Cd^2+

Co^2+ cobalt (II) ion

Cu^2+ copper (II) ion

Fe^2+ iron (II) ion

Mn^2+ manganese (II) ion

Hg2^2+ mercury (II) ion

Ni^2+ nickle (II) ion

Pb^2+ lead (II) ion

Sn^2+ tin (II) ion

Front 21

Ions with 3+ charges.

Back 21

Al^3+ aluminum ion

Cr^3+ chromium (III) ion

Fe^3+ iron (III) ion

Front 22

Ammonium ion

Back 22

NH4^+

Front 23

NH4^+

Back 23

Ammonium ion

Front 24

Cu^+

Back 24

Cooper (I) or cuprous ion

Front 25

Cr^3+

Back 25

Chromium (III) or chromic ion

Front 26

Mass of 1 amu

Back 26

1.66054x10^-22 g

Front 27

Mass of a proton, neutron, and electron, respectively in amu.

Back 27

1.0073amu, 1.0087amu, 5.486x10^-4amu

Front 28

How many amu are in one gram?

Back 28

6.02214x10^23 amu

Front 29

Group 1A name and elements

Back 29

Alkaline metals: Li, Na, K, Rb, Cs, Fr

Front 30

2A group name and elements

Back 30

Alkaline earth metals: Be,Mg,Ca,Sr,Ba,Ra

Front 31

6A group name or elements

Back 31

Chalcogens: O,S,Se,Te,Po

Front 32

7A group name and elements

Back 32

Halogens: F,Cl,Br,I,At

Front 33

8A group name and elements

Back 33

Nobel gases: He, Ne, Ar, Kr, Xe, Rn

Front 34

OH^-

Back 34

Hydroxide ion

Front 35

CN^-

Back 35

Cyanide ion

Front 36

O2^2-

Back 36

Peroxide ion

Front 37

Oxyanions, difference between the -ate and -ite endings

Back 37

Polyatomic anions containing oxygen have names ending in either -ate or -ite.

-ate: used for the most common or representative oxyanion of an element, and -ite is used for an oxyanion

Front 38

Mercury (I) ion

Back 38

Hg2^2+

Front 39

Hg2^2+

Back 39

Mercury (I) ion

Front 40

NO3^-

Back 40

Nitrate ion

Front 41

Nitrate ion

Back 41

NO3^-

Front 42

NO2^-

Back 42

Nitrite ion

Front 43

Nitrite ion

Back 43

NO2^-

Front 44

SO4^2-

Back 44

Sulfate ion

Front 45

Sulfate ion

Back 45

SO4^2-

Front 46

Sulfite ion

Back 46

SO3^2-

Front 47

SO3^2-

Back 47

Sulfite ion

Front 48

ClO4^-

Back 48

Perchlorate ion (1 more O atom than chlorate)

Front 49

Perchlorate

Back 49

ClO4^-

Front 50

ClO3^-

Back 50

Chlorate ion

Front 51

Chlorite ion

Back 51

ClO2^-

Front 52

ClO2^-

Back 52

Chlorite ion (1 O atom fewer than chlorate)

Front 53

Hypochlorite ion

Back 53

ClO^-

Front 54

ClO^-

Back 54

Hypochlorite ion (1 fewer O atom than chlorite)

Front 55

Maximum number of O atoms on polyatomic ions in period 2

Back 55

3

Front 56

Carbonate ion

Back 56

CO3^2-

Front 57

CO3^2-

Back 57

Carbonate ion

Front 58

Phosphate ion

Back 58

PO4^3-

Front 59

PO4^3-

Back 59

Phosphate ion

Front 60

Perchlorate ion

Back 60

ClO4^-

Front 61

Oxyions charge and number of oxygen relation on period table.

Back 61

Front 62

CO3^2-

Back 62

Carbonate ion

Front 63

CO3^2-

Back 63

Carbonate ion

Front 64

HCO3^-

Back 64

Hydrogen carbonate ion (or bicarbonate ion)

Front 65

Hydrogen carbonate ion

Back 65

HCO3^-

Front 66

Phosphate ion

Back 66

PO4^3-

Front 67

PO4^3-

Back 67

Phosphate ion

Front 68

H2PO4^-

Back 68

Dihydrogen phosphate ion

Front 69

H2PO4^-

Back 69

Dihydrogen phosphate ion

Front 70

Acetate ion

Back 70

CH3COO^- or C2H3O2

Front 71

CH3COO^-

Back 71

acetate ion

Front 72

Permanganate ion

Back 72

MnO4^-

Front 73

MnO4^-

Back 73

Permanganate ion

Front 74

CrO4^2-

Back 74

Chromate ion

Front 75

Chromate ion

Back 75

CrO4^2-

Front 76

Dichromate ion

Back 76

Cr2O7^2-

Front 77

Nitride ion

Back 77

N^3-

Front 78

Nitride ion

Back 78

N^3-

Front 79

Define an acid for chemical purposes

Back 79

Is a substance whose molecules yield hydrogen ions when dissolved in water.

Front 80

Naming acids whose anions end in -ide

Back 80

Add hydro- to beginning and -ic acid to the end.

Chloride (Cl^-) becomes hydrochloric acid(HCl)

Sulfide (S^-) becomes hydrosulfuric acid (H2S)

Front 81

Naming acids whose anions end in -ate

Back 81

Change -ate to -ic then add the word acid.

Perchlorate (ClO4^-) becomes perchloric acid (HClO4)

Chlorate (ClO3^-) becomes chloric acid (HClO3)

Front 82

Naming acids whose anions name end in -ite

Back 82

Change -ite to -ous and add the word acid.

Chlorite(ClO2^-) to chlorous acid(HClO2)

Hypochlorite (ClO^-) to hypochlorous acid (HClO)

Front 83

Prefixes for naming binary compounds formed between two nonmetals.

Back 83

Mono- 1

Di- 2

Tri- 3

Tetra- 4

Penta- 5

Hexa- 6

Hepta- 7

Octa- 8

Nona- 9

Deca- 10

Front 84

Procedure for naming binary molecular compounds.

Back 84

1. The name of the element farther to the left in the periodic table is usually written first. Except when the compound contains oxygen and chlorine, bromine, or iodine then oxygen is written last.

2. If both elements are in the same group, the one closer to the bottom of the table is written first.

3. The name of the second element is given an -ide ending.

4. Greek prefixes indicate the number of atoms of each element. When the prefix ends in a or o and the name of the second element begins with a vowel, the a or o of the prefix is dropped.

Front 85

Hydrocarbons

Back 85

Compounds that only contain carbon and hydrogen.

Front 86

Alkanes

Back 86

Simplest hydrocarbons. Each carbon is bonded to four other atoms. The smallest alkane is methane then ethane, and propane.

Front 87

Methane

Back 87

CH4

Front 88

Ethane

Back 88

C2H6

Front 89

C3H8

Back 89

Propane

Front 90

An alcohol

Back 90

An alkane with a -OH group instead of a H

Front 91

Be (chemical name)

Back 91

Beryllium

Front 92

Beryllium chemical symbol

Back 92

Be

Front 93

Rb element name and group

Back 93

Rubidium, alkaline metal

Front 94

Rubidium chemical symbol

Back 94

Rb^1+

Front 95

Cs element name and group

Back 95

Caesium, alkaline metal

Front 96

Br element name and group

Back 96

Bromine, halogen

Front 97

Rn element name and group

Back 97

Radon (noble gas)

Front 98

At element name and group

Back 98

Astatine, halogen

Front 99

Se element name and group

Back 99

Selenium, nonmetal

Front 100

Se element name and group

Back 100

Selenium, nonmetal

Front 101

B element name and group

Back 101

Boron, metalloid

Front 102

Te element name and designation

Back 102

Tellurium, metalloid

Front 103

Sb element name and designation

Back 103

Antimony, metalloid

Front 104

Ge element name and designation

Back 104

Germanium, metalloid

Front 105

Ge element name and designation

Back 105

Germanium, metalloid

Front 106

Sr element name and designation

Back 106

Strontium, alkaline earth metal

Front 107

Sr element name and designation

Back 107

Strontium, alkaline earth metal

Front 108

Ba element name and designation

Back 108

Barium, alkaline earth metal

Front 109

Ra element name and designation

Back 109

Radium, alkaline earth metal

Front 110

How many decimal points do you round the answer when finding the atomic mass of an element based on the abundance and weight of the isotopes?

Back 110

2 decimal points because last function is addition.

Front 111

How many decimal points do you round the answer when finding the atomic mass of an element based on the abundance and weight of the isotopes?

Back 111

2 decimal points because last function is addition.

Front 112

What do you call the rows and columns in the periodic table?

Back 112

Rows are periods, columns are groups.

Front 113

Which elements are the metalloids?

Back 113

Ge, Sb, Po.

Front 114

Which elements are the metalloids?

Back 114

Ge, Sb, Po.

Front 115

What kind of bond holds molecules?

Back 115

Covalent bond (shared electron)/ molecular bond between non-metals and or metalloids.

Front 116

What is an ionic bond?

Back 116

Attraction between two atoms of opposite charge, like Na+ and Cl-.

Front 117

Hypophosphite ion

Back 117

PO2^3-

Front 118

Phosphite ion

Back 118

PO3^2-

Front 119

PO3^2-

Back 119

Phosphite ion

Front 120

PO2^3-

Back 120

Hypophosphite ion

Front 121

IO3^-

Back 121

Iodate

Front 122

Iodate

Back 122

IO3^-

Front 123

Iodite ion

Back 123

IO2^-

Front 124

What did the metal foil scattering alpha particles lead to the discovery of? And replaced what?

Back 124

The nuclear model. The currant pudding model.