Module 4 Test

Question 1

What were categories in Lavoisier’s Table of Simple Substances?

Answer 1

Metals and nonmetals

Question 2

What significantly helped chemists organize the many facts associated with the elements?

Answer 2

Agreeing on how to determine atomic masses

Question 3

Who noticed that by arranging the elements in order of increasing atomic mass, their properties repeated every eighth element?

Answer 3

John Newlands

Question 4

What were features of Mendeleev’s periodic table?

Answer 4

Blank spaces predicted elements yet to be discovered

Elements in columns had similar properties

Question 5

Moseley improved the periodic table by arranging the elements in order of atomic _____ rather than atomic _____.

Answer 5

Number, mass

Question 6

About how many the chemical elements were known by 1870?

Answer 6

Over 60

Question 7

Chemists were better able to organize facts about the elements after they agreed upon a method for accurately determining the atomic _____ of the elements

Answer 7

Mass

Question 8

When John Newlands arranged the elements by atomic mass, he noticed that their properties repeated every
_____ element.

Answer 8

Eighth

Question 9

What is the periodic repetition of properties when the elements are arranged by increasing atomic number?

Answer 9

Periodic law

Question 10

Arrange the statements relating to the development of the periodic table in chronological order.

Answer 10

Elements arranged by increasing atomic mass
Repetition noticed in properties of every eighth element
Existence and properties of undiscovered elements predicted
Discovered that atoms contain a unique number of protons called the atomic number
Elements arranged in order of increasing atomic number

Question 11

Moseley improved the pattern of properties in the periodic table by arranging elements by ______.

Answer 11

Atomic number

Question 12

What events played major roles in the advancing the number of known elements?

Multiple select question.

Answer 12

Advent of electricity

Development of the spectrometer

The industrial revolution

Question 13

The statement that there is a periodic repetition of properties of the elements when they are arranged by increasing atomic number is called the ____ ____.

Answer 13

Periodic Law

Question 14

The modern periodic table consists of boxes, each containing an element name, symbol, atomic ____, and atomic ____.

Answer 14

Number, mass

Question 15

What scientists contributed to the development of the periodic table?

Answer 15

Henry Moseley
Dmitri Mendeleev
John Newlands
Lothar Meyer

Question 16

What are key features of the modern periodic table?

Answer 16

1. The elements in groups 3 to 12 are called the transition elements.
2. The boxes are arranged into a series of columns, called groups or families, and rows, called periods.
3. The elements in groups 1, 2, and 13 to 18 are referred to as the main group, or representative elements.
4. It consists of boxes, each containing an element name, symbol, atomic number, and atomic mass.

Question 17

What is a vertical column of elements in the periodic table arranged in order of increasing atomic number?

Answer 17

Group

Question 18

What elements have been known since prehistoric times?

Answer 18

Carbon
Gold
Silver

Question 19

What is a horizontal row of elements in the modern periodic table?

Answer 19

Period

Question 20

The elements in groups 1, 2, and 13 to 18 possess a wide range of chemical and physical properties. For this reason, they are often referred to as the main group elements or what other term?

Answer 20

Representative elements

Question 21

What term describes the elements in groups 3 through 12 on the periodic table?

Answer 21

Transition elements

Question 22

What were categories in Lavoisier’s Table of Simple Substances?

Answer 22

Metals
Nonmetals
Gases
Earths

Question 23

What are elements that are generally shiny when smooth and clean, solid at room temperature, and good conductors of heat and electricity?

Answer 23

Metals

Question 24

What are examples of metals?

Answer 24

calcium (Ca)

sodium (Na)

mercury (Hg)

lithium (Li)

Question 25

Elements in groups 3 through 12 (with the exception of the lanthanide series and actinide series) are called the _____ metals.

Answer 25

Transition

Question 26

The transition elements included in the lanthanide series and actinide series are called the _____ transition metals.

Answer 26

Inner

Question 27

What are the transition elements (with the exception of the lanthanide series and actinide series) located in groups 3 through 12 on the periodic table?

Answer 27

Transition metals

Question 28

Elements 57 through 71 in the sixth period are known as the ______ series.

Answer 28

Lanthanide

Question 29

What term refers to elements 89 through 103 in the seventh period of the periodic table?

Answer 29

Actinide series

Question 30

What are examples of nonmetals?

Answer 30

carbon (C) radon (Rn) helium (He) bromine (Br)

Question 31

What term refers to the lanthanide series and actinide series, located at the bottom of the periodic table?

Answer 31

Inner transition metals

Question 32

What is the group of elements that are generally gases or brittle, dull looking solids, and poor conductors of heat and electricity?

Answer 32

Nonmetals

Question 33

The highly reactive elements in group 17 of the periodic table are known as ____.

Answer 33

Halogens

Question 34

What term describes the extremely unreactive group 18 gases? Multiple choice question.

Answer 34

Noble gases

Question 35

Many nonmetals have interesting properties and applications. For example, the only nonmetal that is a liquid at room temperature is _______ the most abundant element in the human body is the nonmetal _____ and the element commonly added to toothpaste and drinking water to prevent tooth decay is ______

Answer 35

Bromine Oxygen Fluorine

Question 36

What are examples of metalloids?

Answer 36

antimony (Sb) germanium (Ge) arsenic (As) silicon (Si)

Question 37

What are elements that have the physical and chemical properties of both metals and nonmetals?

Answer 37

Metalloids

Question 38

Elements in the same group have similar chemical properties because they have the same _____ __ ______ _______.

Answer 38

number of valence electrons

Question 39

Two important metalloids that are used extensively in computer chips and solar cells are _____ and ______.

Answer 39

Silion, germanium

Question 40

The energy level of an element's valence electrons indicates the _____ on the periodic table in which it is found.

Answer 40

Period

Question 41

What can be determined from the period in which an element appears on the periodic table?

Answer 41

energy level of valence electrons

Question 42

The group 18 elements are extremely stable because the ___ and ____ orbitals are completely filled.

Answer 42

S, P

Question 43

The periodic table is divided into sections, or blocks, representing the atom’s energy sublevel being filled with valence electrons. These are known as the ___, ____, ___, and _____ blocks.

Answer 43

S, P, D, F

Question 44

What characterize the electron configurations of the d-block elements?

Answer 44

filled outermost s orbital of energy level n filled or partially filled d orbitals of energy level n – 1

Question 45

What explains the stability of the electron configurations of the group 18 elements?

Answer 45

The s and p orbitals are completely filled.

Question 46

Elements in the f-block of the periodic table are characterized by a filled or partially filled outermost ____ orbital and filled or partially filled 4f and 5f orbitals.

Answer 46

S

Question 47

Most d-block elements in period 4 have partially filled d orbitals of energy level ____.

Answer 47

3

Question 48

For metals such as sodium, atomic radius is defined as

Answer 48

half the distance between nuclei in a crystal of the element.

Question 49

What is an observed trend in atomic radii?

Answer 49

atomic radii decrease across a period from left to right

Question 50

Atomic radii decrease across a period because the valence electrons are all in the same energy level but are attracted more strongly by the greater number of _____ in the nucleus.

Answer 50

Protons

Question 51

What is an observed trend in atomic radii?

Answer 51

atomic radii increase down a group

Question 52

Atomic radii generally increase moving down a group because the increased distance of valence electrons from the nucleus offsets the pull of the increased _____ charge.

Answer 52

Positive

Question 53

In general, there is a(n) ______ in atomic radii as you move from left to right across a period.

Answer 53

decrease

Question 54

What are reasons for atomic radii decreasing across a period?

Answer 54

no new energy levels are added more protons are added to the nucleus no additional electrons come between the valence electrons and the nucleus

Question 55

An atom or group of bonded atoms that has a positive or negative charge is called a/an ____.

Answer 55

ion

Question 56

Atoms always become smaller when they _____ electrons and form ions with a _____ charge.

Answer 56

Lose, positive

Question 57

What factors explain why atomic radii generally increase when moving down a group?

Answer 57

electrons in inner orbitals shield the outer electrons from the nucleus increased distance of valence electrons from the nucleus offsets the pull of increased nuclear charge added principal energy levels are farther from the nucleus

Question 58

An atom that gains an electron and forms an ion with a ______ charge becomes _____ in size.

Answer 58

Negative, bigger

Question 59

Moving across a period, the change from positive to negative ions causes a sudden _____ in ionic radii at group 15 or 16.

Answer 59

Growth

Question 60

How do ionic radii vary moving down a group?

Answer 60

Both positive and negative ionic radii increase.

Question 61

True or false: Atoms always become larger when they lose electrons and form positively charged ions.

Answer 61

False

Question 62

Why is this false: Atoms always become larger when they lose electrons and form positively charged ions.

Answer 62

They become smaller because losing a valence electron results in a completely empty outer orbital or in valence electrons experiencing less electrostatic repulsion and therefore a greater nuclear charge.

Question 63

The energy required to remove an electron from a gaseous atom is called the ______ energy.

Answer 63

Ionization

Question 64

Atomic radii generally increase moving down a group because the increased distance of valence electrons from the nucleus offsets the pull of the increased _____ charge.

Answer 64

Positive

Question 65

When atoms gain electrons, they ______.

Answer 65

form negatively charged ions and become larger

Question 66

What of these are correct descriptions of trends in ionic radii moving from left to right across a period?

Answer 66

radii of negative ions decrease radii increase at the dividing line between positive and negative ions radii of positive ions decrease

Question 67

Ionic radii of both positive and negative ions ____ moving down a group.

Answer 67

Increase

Question 68

What are characteristics of atoms with high ionization energy?

Answer 68

They are unlikely to form positive ions. They have a strong hold on electrons.

Question 69

What factors explain why atomic radii generally increase when moving down a group?

Answer 69

electrons in inner orbitals shield the outer electrons from the nucleus added principal energy levels are farther from the nucleus increased distance of valence electrons from the nucleus offsets the pull of increased nuclear charge

Question 70

The third ionization energy is the energy required to remove ______.

Answer 70

one electron from a 2+ ion

Question 71

How do ionic radii vary moving down a group?

Answer 71

Both positive and negative ionic radii increase.

Question 72

Ionization energy generally _____ across a period.

Answer 72

Increases

Question 73

Atoms that have a low ionization energy are likely to form ______ ions.

Answer 73

Positive

Question 74

What explains the decrease in ionization energy moving down a group?

Answer 74

The valence electrons are farther from the nucleus.

Question 75

True or false: For a given atom, the second ionization energy is always less than the first ionization energy.

Answer 75

False

Question 76

Why is this false: For a given atom, the second ionization energy is always less than the first ionization energy.

Answer 76

Each successive electron requires more energy to remove than the previous one.

Question 77

When atoms gain electrons, they ______.

Answer 77

form negatively charged ions and become larger

Question 78

Which rule states that atoms tend to gain, lose, or share electrons in order to acquire a full set of eight valence electrons?

Answer 78

octet rule

Question 79

The relative ability of atoms to attract electrons in a chemical bond is called ______.

Answer 79

Electronegativity

Question 80

True or false: Electronegativity increases moving down a group.

Answer 80

False

Question 81

Why is this false: Electronegativity increases moving down a group.

Answer 81

Electronegativity decreases moving down a group because electrons are farther from the nucleus.

Question 82

What did John Newlands do?

Answer 82

He discovered the law of octaves

Question 83

What did Mendeleev contribute to the periodic table?

Answer 83

He provided the base to organize the elements on the table, predicted undiscovered elements

Question 84

What is the periodic table?

Answer 84

A table that organizes elements by their properties

Question 85

Elements in groups 3-12 are called?

Answer 85

Transition metals

Question 86

Elements on the periodic table are in order of increasing _____?

Answer 86

Both atomic number and number of protons

Question 87

Mendeleev organized his periodic table according to what?

Answer 87

Atomic mass

Question 88

Elements with similar outer electron configurations have what in common?

Answer 88

They have similar reactivities because they have similar numbers of valence electrons

Question 89

Why are alkali metals so reactive?

Answer 89

They have exactly one electron on their outer shell

Question 90

What are metalloids?

Answer 90

Semi-conductors

Question 91

Where are metalloids located?

Answer 91

They are located along the "staircase"

Question 92

Is Ge a metal, nonmetal, or metalloid?

Answer 92

Metalloid

Question 93

Is Na a metal, nonmetal, or metalloid?

Answer 93

Metal

Question 94

Is Xe a metal, nonmetal, or metalloid?

Answer 94

Nonmetal

Question 95

Is Rn a metal, nonmetal, or metalloid?

Answer 95

Nonmetal

Question 96

What is electron shielding?

Answer 96

Inner electrons shield the valence electrons on the shell from protons or the nucleus

Question 97

Elements in the same group on the periodic table have similar?

Answer 97

Properties

Question 98

Groups on the periodic table are arranged?

Answer 98

Vertically

Question 99

The rows of a periodic table are called?

Answer 99

Periods

Question 100

What is a Lewis dot diagram?

Answer 100

A diagram showing the number of valence electrons

Question 101

Electron affinity is?

Answer 101

The amount of energy required to add an electron to an atom

Question 102

Electronegativity is?

Answer 102

The measure of the tendency to attract electrons

Question 103

Ionization energy is?

Answer 103

The amount of energy needed to remove an electron from the atom