Ch 6: The Periodic Table

Question 1

Chemists use the __________ of elements to sort them into ______.

Answer 1

properties

groups

Question 2

Who published a classification system in which he grouped elements into triads?

Answer 2

J. W. Dobereiner

Question 3

Who arranged the elements in his periodic table in order of increasing atomic mass?

Answer 3

Mendeleev

Question 4

How are elements arranged in the modern periodic table?

Answer 4

In order of increasing atomic number.

Question 5

What are the three classes of elements?

Answer 5

1. Metals
2. Nonmetals
3. Metalloids

Question 6

The periodic table displays the _______ and _____ of the elements along with information about the _________ of their atoms.

Answer 6

symbols
names
structure

Question 7

Elements can be sorted into _____ _____, ______________ ________, __________ ______, or _____ __________ ______ based on their electron configuration.

Answer 7

noble gases
representative elements
transition metals
inner transition metals

Question 8

What is the distance from the nucleus to the furthermost electron referred to as?

Answer 8

Atomic radius

Question 9

In general, atomic size _________ from top to bottom within a group and _________ from left to right across a period.

Answer 9

increases

decreases

Question 10

Atomic radius: largest value

Answer 10

Bottom left

Question 11

Atomic radius: smallest value

Answer 11

Top right

Question 12

Atomic radius: group trends

Answer 12

The amount of energy levels is increasing.

Question 13

Atomic radius: periodic trends

Answer 13

Gaining protons.

Question 14

Positive and negative ions form when _________ are transferred between atoms.

Answer 14

electrons

Question 15

What is the amount of energy needed to remove the most loosely held electron referred to as?

Answer 15

Ionization energy

Question 16

Ionization energy tends to ________ from top to bottom within a group and ________ from left to right across a period.

Answer 16

decrease

increase

Question 17

Ionization energy: largest value

Answer 17

Top right

Question 18

Ionization energy: smallest value

Answer 18

Bottom left

Question 19

Ionization energy: group trends

Answer 19

Farther from the nucleus, electron is easier to lose.

Question 20

Ionization energy: periodic trends

Answer 20

The atoms are getting smaller/closer to the nucleus.

Question 21

Cations are always _______ than the atoms from which they form. Anions are always ______ than the atoms from which they form.

Answer 21

smaller

larger

Question 22

Metals form positively charged ions by ______ electrons.

Answer 22

Losing

Question 23

Cations: groups

Answer 23

Increase ionic radius

Question 24

Cations: periods

Answer 24

Decrease ionic radius

Question 25

Nonmetals form negatively charged ions by _______ electrons.

Answer 25

Gaining

Question 26

Anions: groups

Answer 26

Decrease ionic radius

Question 27

Anions: periods

Answer 27

Increase then decrease ionic radius

Question 28

What is the relative attractiveness an atom has for its shared electrons?

Answer 28

Electronegativity

Question 29

Electronegativity values ________ from top to bottom with a group.

Answer 29

Decrease

Question 30

Why does electronegativity decrease from top to bottom?

Answer 30

Farther from the nucleus.

Question 31

For representative elements, the values tend to ________ from left to right across a period.

Answer 31

Increase

Question 32

Why does representative element values increase from left to right?

Answer 32

Closer to the nucleus.

Question 33

Representative elements: largest value

Answer 33

Top right

Question 34

Representative elements: smallest value

Answer 34

Bottom left

Question 35

The trends that exist among these properties can be explained by variations in ______ _________.

Answer 35

atomic structure