Periodic Table And Energy

Question 1

What are the vertical column in the periodic table called?

Answer 1

Groups

They have same number of outer shell electrons and similar properties.

Question 2

What are the horizontal rows in a periodic table called?

Answer 2

Periods

The number of the period gives the number of the highest energy electron shells in an element’s atoms.

Question 3

What does ionisation energy measure?

Answer 3

How easily an atom loses electrons to form positive ions.

Question 4

Definition the first ionisation energy?

Answer 4

The energy required to remove one electron from each atom in one mole of gaseous atoms of an element to form one moles of gaseous 1+ ions.

Question 5

What factors affect ionisation energy?

Answer 5

Atomic radius
Nuclear charge
Electron shielding

Question 6

How does atomic radius affect ionisation energy?

Answer 6

The greater the distance between the nucleus and the outer electrons, the less the nucleus attraction. The force of attraction fall

Question 7

How does nuclear charge affect ionisation energy?

Answer 7

The more protons there are in the nucleus of an atom, the greater the attraction, between the nucleus and the outer electrons.

Question 8

How does electron shielding?

Answer 8

Electrons are negatively charged and so inner-shell electrons repel outer-she’ll electrons. This repulsion, called the shielding effect, reduces the attraction between the nucleus and the outer electrons.

Question 9

What is an ionised gas called?

Answer 9

Plasma

Question 10

What is the second ionisation energy definition

Answer 10

The energy required to remove one electron from ion in one mole of gaseous 1+ ions of an element to form one mole of gaseous 2+ ions.

Question 11

What is the trend down a group in first ionisation energies?

Answer 11

Atomic radius increases
More inner shells so shielding increases
Nuclear attraction on outer electrons decreases
First ionisation energy decreases.

Question 12

What are the trends across a period in first ionisation energies?

Answer 12

Nuclear charge increases 
Same shell; similar shielding
Nuclear attraction increases
Atomic radius decreases
First ionisation energy increases

Question 13

Why is there a fall in the first ionisation energies from beryllium to boron?

Answer 13

2p sub shell is beginning to be filled

Question 14

What is one constant property of metals?

Answer 14

Their ability to conduct electricity.

Question 15

What is a cation?

Answer 15

A positively charged ion with fewer electrons than protons.

Question 16

What is an anion?

Answer 16

A negatively charged ion with more electrons than protons

Question 17

Name some properties of metals

Answer 17

Strong metallic bonds-attraction between positive ions and delocalised electrons.
High electrical conductivity
High melting and boiling points

Question 18

Are metals soluble?

Answer 18

No

Question 19

What are typical properties of substances with giant covalent structures?

Answer 19

Very strong covalent bonds so are very stable and hard to break down.

Question 20

What are the melting and boiling points of giant covalent lattices?

Answer 20

They are very high- this is because covalent bonds are strong. High temperatures are necessary to provide the large quantity of energy to break the bonds.

Question 21

How soluble are giant covalent lattices?

Answer 21

Insoluble in almost all solvents. The covalent bonds are too strong to be broken by interactions with solvents.

Question 22

Are giant covalent lattices conductors of electricity?

Answer 22

They already mostly non-conductors, however graphemes and graphite are exceptions.

Question 23

What is the trend in melting points across the period?

Answer 23

Melting point increases from group 1 to group 14.
There is a sharp decrease between group 14 and group 15 this is because of a change from giant to simple molecular structures.
The melting points are low from group 15 to group 18.

Question 24

What are the characteristics of group 2 elements?

Answer 24

Metals
Reactive
Often found as a compound rather than pure

Question 25

Are group 2 metals reducing agents?

Answer 25

Yes they are oxidised and reduce another species.

Question 26

What do group 2 elements form when they react with oxygen?

Answer 26

Metal oxide