Periodic Table - Term 2

Question 1

Which of the following takes up majority of the Periodic Table?

A. Metalloids
B. Non-Metals
C. Metals

Answer 1

C. Metals

Question 2

Which of the following “subheadings” takes up the middle of the Periodic Table?

A. Alkali Metals
B. Transition Metals
C. Rare Earth Elements

Answer 2

B. Transition Metals

Question 3

Do periods go across or down the Periodic Table?

Answer 3

Across

Question 4

Do groups go across or down the Periodic Table?

Answer 4

Down

Question 5

Which of the following are involved in covalent bonding?

A. Non-Metals
B. Metals

Answer 5

A. Non-Metals

Question 6

Do atoms increase or decrease in size across the period? Why?

Answer 6

Atoms decrease across the period, due to the increasing nuclear charges. As the nuclear charge increases, the electrons are pulled closer to the nucleus, decreasing the radius and therefore making the atom smaller.

Question 7

Do atoms increase and decrease in size down the group? Why?

Answer 7

Atoms increase in size down the group, due to the increasing number of electron shells. These electron shells shield the nucleus from the valence electrons and push the valence shell further away from the nucleus, resulting in an increased radius and larger atom.

Question 8

Positive ions are called …

Answer 8

Cations

Question 9

Negative ions are called …

Answer 9

Anions

Question 10

An ION is an atom that has …

Answer 10

Lost or gained electrons

Question 11

A cation forms when an atom ____ electrons

Answer 11

Loses

Question 12

An anion forms when an atom ____ electrons

Answer 12

Gains

Question 13

Is the ionic radius of a cation smaller/larger than that of it’s atom? Why/why not?

Answer 13

Smaller, because atoms that become cations lose their valence electrons, meaning they lose an entire shell to become stable, whereas the atom keeps it’s valence shell.

Question 14

Species with the name numbers of electrons are called …

Answer 14

Isoelectronic

Question 15

Ionization energy is …

Answer 15

The energy required to remove an electron.

Question 16

What is the general trend in ionization energy across a period?

Answer 16

The ionization energy increases across a period.

Question 17

What is the definition of second ionization energy?

Answer 17

The energy required to remove a second electron.

Question 18

What is the definition of third ionization energy?

Answer 18

The energy required to remove a third electron.

Question 19

What is electronegativity?

Answer 19

The ability of an atom to attract nearby electrons.

Question 20

What atom has the highest electronegativity?

Answer 20

Flourine

Question 21

Which element has the lowest electronegativity?

Answer 21

Francium

Question 22

What TWO factors influence electronegativity?

A. Amount of electron shells (atom size)
B. Nuclear charge
C. Atom colour

Answer 22

A. Amount of electron shells (atom size)
B. Nuclear charge

Question 23

Does electronegativity increase/decrease across a period? Why/why not?

Answer 23

Electronegativity increases across the period. This is due to the increasing nuclear charge and decreasing atomic radius.

Question 24

Does electronegativity increase/decrease down a group? Why/why not?

Answer 24

Electronegativity decreases down the group. This is due to the increasing atomic size and increased shielding affect.

Question 25

The difference in electronegativity tells us what kind of bonding the compound will have. True/False?

Answer 25

True

Question 26

Which of the following tells you how many valence electrons the element has?

A. The group
B. The period

Answer 26

A. The group

Question 27

Do Lewis Dot Diagrams show all the electrons or just the valence electrons?

Answer 27

Just the valence electrons.

Question 28

Noble gases are stable. True/False

Answer 28

True