Chapter 2

Question 1

the smallest identifiable unit of an element

Answer 1

atom

Question 2

the matter that reacts

Answer 2

reactants

Question 3

the matter that forms

Answer 3

product

Question 4

The theory that all matter is composed of
atoms originated from several observations
and laws.

Answer 4

atomic theory

Question 5

In a chemical reaction, matter is neither
created nor destroyed.

Answer 5

law of conservation of mass

Question 6

law of conservation of mass

Answer 6

In a chemical reaction, matter is neither
created nor destroyed.

Question 7

All samples of a given compound, regardless of
their source or how they were prepared, have the
same proportions of their constituent elements.

Answer 7

Law of definite proportions

Question 8

When two elements (call them A and B) form
two different compounds, the mass of element
B that combine with 1 g of element A can be
expressed as a ratio of small whole numbers.

Answer 8

Law of multiple proportions

Question 9

partially evacuated glass
tube called a

Answer 9

cathode ray tube

Question 10

a beam of particles

Answer 10

cathode rays

Question 11

negatively charged electrode

Answer 11

cathode

Question 12

positively charged electrode

Answer 12

anode

Question 13

a fundamental property of some of the particles that compose atoms and results in attractive and repulsive forces between hose particles

Answer 13

electrical charge

Question 14

attractive and repulsive forces

Answer 14

electrostatic forces

Question 15

the area around a charged particle

Answer 15

electric field

Question 16

fundamental charge

Answer 16

–1.6 × 10–19

Question 17

proposed that the negatively
charged electrons were small particles held
uniformlywithin a positively charged
sphere.

Answer 17

J.J. Thomson

Question 18

directed
positively charged particles at an ultra thin
sheet of gold foil.

Answer 18

Ernest Rutherford

Question 19

what did oil drop experiment do

Answer 19

deduce that the charge of a single electron

Question 20

what did oil drop experiment do

Answer 20

deduce that the charge of a single electron Z

Question 21

the emission of small energetic particles from the core of certain unstable atoms

Answer 21

radioactivity

Question 22

a small core called a

Answer 22

nucleus

Question 23

positively charged particles

Answer 23

protons

Question 24

neutral particles within the nucleus

Answer 24

neutrons

Question 25

the mass of a proton

Answer 25

1.67493 x 10 to the negative 27th power kg`

Question 26

the mass of a neutron

Answer 26

1.67493 x 10 to the negative 27th power kg`

Question 27

the mass of an electron

Answer 27

9.1 x 10 to the negative 31st power kg

Question 28

unit to express the mass

Answer 28

atomic mass units (amu)

Question 29

the most important number to identify an atom is

Answer 29

the number of protons

Question 30

The number of protons in an atom’s nucleus is its

Answer 30

atomic number

Question 31

what is the symbol fo 4th atomic number

Answer 31

Z

Question 32

He

Answer 32

Helium

Question 33

Helium

Answer 33

He

Question 34

H

Answer 34

Hydrogen

Question 35

Hydrogen

Answer 35

H

Question 36

Li

Answer 36

Lithium

Question 37

Lithium

Answer 37

Li

Question 38

Be

Answer 38

Beryllium

Question 39

Beryllium

Answer 39

Be

Question 40

B

Answer 40

Boron

Question 41

Boron

Answer 41

B

Question 42

C

Answer 42

carbon

Question 43

Carbon

Answer 43

C

Question 44

N

Answer 44

Nitrogen

Question 45

Nitrogen

Answer 45

N

Question 46

O

Answer 46

Oxygen

Question 47

Fluorine

Answer 47

F

Question 48

Neon

Answer 48

Ne

Question 49

Sodium

Answer 49

Na

Question 50

Magnesium

Answer 50

Mg

Question 51

Aluminum

Answer 51

Al

Question 52

Silicon

Answer 52

Si

Question 53

Phosphorus

Answer 53

P

Question 54

Sulfer

Answer 54

S

Question 55

Chlorine

Answer 55

Cl

Question 56

Argon

Answer 56

Ar

Question 57

potassium

Answer 57

K

Question 58

Calcium

Answer 58

Ca

Question 59

is either a one- or two-letter abbreviation listed directly below its atomic number on the periodic table.

Answer 59

chemical symbol

Question 60

toms with the same number of protons but a different number of neutrons are called

Answer 60

isotopes

Question 61

The relative amount of each isotope in a naturally occurring sample of a given element is roughly constant.

Answer 61

natural abundance

Question 62

this has allowed accurate measurements that reveal small but significant variations in the natural abundance of isotopes for many elements.

Answer 62

mass spectrometry

Question 63

The sum of the number of neutrons and protons in an atom is its

Answer 63

mass number

Question 64

symbol for chemical symbol

Answer 64

X

Question 65

Symbol for mass number

Answer 65

A

Question 66

Atoms can lose or gain electrons and become charged particles

Answer 66

ions

Question 67

Atoms can lose or gain electrons and become charged particles

Answer 67

ions

Question 68

positively charges ions

Answer 68

cations

Question 69

Negatively charged ions

Answer 69

anions

Question 70

what is the law of periodic law

Answer 70

When the elements are arranged in order of increasing atomic mass, certain sets of properties recur periodically.

Question 71

When the elements are arranged in order of increasing atomic mass, certain sets of properties recur periodically.

Answer 71

periodic law

Question 72

Columns are referred to as

Answer 72

groups

Question 73

Rows are called

Answer 73

periods

Question 74

predicted the existence (and even the properties) of yet undiscovered elements.

Answer 74

Mendeleev’s table

Question 75

how are the elements listed in modern table

Answer 75

increasing in atomic number

Question 76

where does metal reside on table

Answer 76

lower left side and middle

Question 77

where do nonmetal lie

Answer 77

in the upper right side of the periodic table

Question 78

how many nonmetals are there

Answer 78

17

Question 79

where do metalloids lie

Answer 79

zigzag diagonal line that divides metals and nonmetals.

Question 80

intermediate (and highly temperature- dependent) electrical conductivity.

Answer 80

semiconductors

Question 81

whose properties tend to be largely predictablebased on their position in the periodic table.

Answer 81

main-group elements

Question 82

whose properties tend to be less predictable based simply on their position in the periodic table.

Answer 82

transition elements or transition metals

Question 83

how Many groups are there

Answer 83

18

Question 84

how many periods are there

Answer 84

7

Question 85

the most unreacted elements

Answer 85

noble gases (8A)

Question 86

the reactive metals

Answer 86

alkali metals (1A)

Question 87

elements within a column are considered

Answer 87

families

Question 88

They are fairly reactive

Answer 88

alkaline earth metals (2A)

Question 89

are very reactive nonmetals.

Answer 89

halogens (7A)

Question 90

always found in nature as a salt

Answer 90

halogens

Question 91

tend to lose electrons, forming a cation with the same number of electrons as the nearest noble gas.

Answer 91

main group metals

Question 92

tend to gain electrons forming an anion with the same number of electrons as the nearest noble gas

Answer 92

main group nonmetals

Question 93

elements in the same what have similar properties

Answer 93

group

Question 94

have a tendency to lose one electron and form 1+ ions.

Answer 94

alkali metals (group 1A)

Question 95

tend to lose two electrons and form 2+ ions.

Answer 95

alkaline earth metals (group 2A) `

Question 96

tend to gain one electron and form 1– ions.

Answer 96

halogens (group 7A)

Question 97

tend to gain two electrons and form 2– ions

Answer 97

oxygen family nonmetals (group 6A)

Question 98

what are main-group elements that form cations

Answer 98

metals

Question 99

what are the main-group elements that form anions (nonmetals) with predictable charge equal to

Answer 99

the group number minus eight

Question 100

average mass of the isotopes that compose that element, weighted according to the natural abundance of each isotope.

Answer 100

atomic mass

Question 101

where is the atomic mass shown

Answer 101

directly beneath the element’s symbol in the periodic table.

Question 102

a technique that separates particles according to their mass.

Answer 102

mass spectrometry

Question 103

The masses of atoms and the percent abundances of isotopes of elements are measured using what

Answer 103

mass spectrometry

Question 104

what does the position of each peak indicate

Answer 104

the mass of the isotopes

Question 105

what dies the intensity (height of the peak) indicate

Answer 105

relative abundance of that isotope

Question 106

where does chemical process happen?

Answer 106

between particles

Question 107

is the amount (g) per mole

Answer 107

molar mass

Question 108

the amount of material containing 6.02214 x 10 to the 23rd particle

Answer 108

mole

Question 109

the number of moles of a substance

Answer 109

the amount of a substance

Question 110

the mass of one mole of an atom of an element is

Answer 110

molar mass

Question 111

An element’s molar mass in grams per mole is numerically equal what

Answer 111

atomic mass units (amu)