Chapter 2

Question 1

Metal properties

Answer 1

o Shiny, malleable, good conductors of heat and electricity

o Tend to lose electrons when they undergo a chemical reactions - cations

Question 2

Nonmetal properties

Answer 2

o Appear dull, poor conductors of heat and electricity

o Tend to gain electrons when they undergo a chemical reaction and become ions

Question 3

Metalloids properties

Answer 3

o Properties between metals and nonmetals

o Semiconductors with intermediate conductivity

Question 4

Family name of group 1 besides Hydrogen

Answer 4

Alkali metals

Question 5

Family name of group 2

Answer 5

Alkaline earth metals

Question 6

Family name of group 3-12

Answer 6

Transitional metals

Question 7

Family name of group 17

Answer 7

Halogens

Question 8

Family name of group 18

Answer 8

noble gases

Question 9

Group 1 charges

Answer 9

1+ charge

Question 10

Group 2 charges

Answer 10

2+ charge

Question 11

Group 17 charges

Answer 11

1- Charge

Question 12

Group 16 charges

Answer 12

2- charge

Question 13

Group 15 charges

Answer 13

3- charge

Question 14

Group 14 charge

Answer 14

4- Charge

Question 15

Aluminum charge

Answer 15

Al 3+

Question 16

4 parts of Dalton’s atomic theory

Answer 16

1. Each element is composed of small particles called atoms
2. all atoms of a given element are identical and different from another element
3. Atoms of one element cannot be changed into a different element by chemical reactions
4. Compounds are formed when atoms of more than one element combine. Always with the same number of atoms

Question 17

Rutherford contributions

Answer 17

1. discovered the nucleus
2. Most of the mass and all positive charges are in the nucleus
3. Most of the volume is in empty space occupied by electrons
4. There are as many negative charged electrons outside the nucleus as units of positive charge inside the nucleus and atom is electronically neutral

Question 18

J.J. Thompson contribution

Answer 18

Discovered the electron using a cathode rays as a stream of electrons

Question 19

Millikan contribution

Answer 19

Determined the charge of an electron using the oil drop experiment

Question 20

James Chadwick

Answer 20

Discovered the neutron

Question 21

Protons calculation and description

Answer 21

Same as the atomic number

Positive

Question 22

Neutrons

Answer 22

Atomic mass - atomic number

Neutral

Question 23

Electrons

Answer 23

Atomic number - charge
Negative
Outside of the nucleus

Question 24

Isotopes characteristics

Answer 24

o Differ in the number of neutrons in nucleus as the atomic mass differ
o Protons is the same in all the isotopes
o Mass spectrometer analyzes the percent of each isotope

Question 25

Calculate atomic mass from the abundance of isotopes

Answer 25

percent x mass of isotope 1 + percent x mass of isotope 2 .. and so on

Question 26

Difference between atomic number, atomic mass and mass number

Answer 26

o Atomic number = the number of protons in an atom. o Atomic mass = The average mass of an atom, considering all its naturally occurring isotopes. Most likely expressed in decimals. o Mass number = The sum of the number of protons and the number of neutrons in an atom. Will be a whole number. This number will vary with isotopes since they have different neutrons.

Question 27

Molecular compounds

Answer 27

- Contains only nonmetals and no ions - Also known as covalent compounds - Atoms share, rather than transfer (gain or lose) electrons - Uses numerical prefixes-

Question 28

Formula steps for binary molecular compounds

Answer 28

o First name the more metallic element o Then name the less metallic element + ide suffix o Use the prefixes for both parts of the name unless there is only one of the first type of atom

Question 29

Binary compounds prefixes Mono

Answer 29

1

Question 30

Binary compounds prefixes Di-

Answer 30

2

Question 31

Binary compounds prefixes Tri -

Answer 31

3

Question 32

Binary compounds prefixes 4 -

Answer 32

Tetra

Question 33

Binary compounds prefixes 5 -

Answer 33

Penta

Question 34

Binary compounds prefixes 6 -

Answer 34

Hexa

Question 35

Binary compounds prefixes Hepta -

Answer 35

7

Question 36

Binary compounds prefixes Octa -

Answer 36

8

Question 37

Binary compounds prefixes Nona -

Answer 37

9

Question 38

Binary compounds prefixes Deca -

Answer 38

10

Question 39

Ionic compounds

Answer 39

Compounds containing a metal and one or more nonmetals Held together by ionic bonds Electrostatic attraction between a cation (metal) and anion (nonmetal

Question 40

When ionic compounds dissolve in water:

Answer 40

Ionic bonds are broken individual cations and anions float around in the water Solutions conducts electricity known as electrolyte solution

Question 41

Ionic compounds formula steps

Answer 41

1. Name the cation (metal) first by its elemental name | 2. Next name the anion (nonmetal) + ide suffix

Question 42

Ionic compounds special rules

Answer 42

Polyatomic anions will keep their name in the iconic compound If the cation (such as a transitional metal) can have more than one possible charge, write the charge as a roman numeral in parentheses

Question 43

Molecular vs ionic compound

Answer 43

Molecular compound will most likely have the prefix and ionic compounds will not Roman numerals: - For metals that can have more than one type of cation - Indicate the charge of the cation (metal) - Anion and its charge are used to deduce the charge of the metal cation to make it neutral

Question 44

Acids formula rules: Anion ends in "ide"

Answer 44

change ending to "ic acid" add the prefix "hydro" ex. hydrochloric acid

Question 45

Acids formula rules: Anion ends in "ate"

Answer 45

change ending to "ic acid" only ex. chloric acid

Question 46

Acids formula rules: Anion ends in "ite"

Answer 46

Change the ending to "-ous acid" Ex. hydrochlorous acid or chlorous acid