8.2- TRENDS IN THE PROPERTIES OF ELEMETNS OF PERIOD 3

Question 1

What does the Periodic Table reveal?

Answer 1

patterns in properties of elements

Question 2

What is an example of periodicity in the Periodic Table?

Answer 2

every time you go across a period you for from metals on left to non-metals on right

Question 3

What does periodic mean?

Answer 3

recurring regularly

Question 4

What is periodicity explained by?

Answer 4

electron arrangement of elements

Question 5

Are elements in group 1, 2 + 3 metals or non-metals?

Answer 5

metals

Question 6

What sort of structure do elements in group 1, 2 + 3 have?

Answer 6

giant structures

Question 7

What do elements in group 1, 2 + 3 do to form ionic compounds?

Answer 7

lose their outer electrons to form ionic compounds

Question 8

How many electrons does silicon in group 4 have in its outer shell?

Answer 8

4 electrons

Question 9

What does silicon do with its outer electrons?

Answer 9

forms four covalent bonds

Question 10

What properties does silicon have?

Answer 10

has some metallic properties

Question 11

What is silicon classed as, as it has some metallic properties?

Answer 11

semi-metal

Question 12

Are the elements in group 5, 6 + 7 metals or non-metals?

Answer 12

non-metals

Question 13

In regards to electrons, what do group 5, 6 + 7 elements do?

Answer 13

either accept electrons to form ionic compounds, or share their outer electrons to form covalent compounds

Question 14

Why is argon unreactive?

Answer 14

its a noble gas in group 0- has full outer shell

Question 15

What structures tend to have high melting + boiling points?

Answer 15

giant structures

Question 16

Where are the elements with giant structures on the Periodic table?

Answer 16

on the left

Question 17

What structures tend to have low melting + boiling points?

Answer 17

molecular or atomic structures

Question 18

Where are the elements with molecular or atomic structures on the Periodic table?

Answer 18

on the right

Question 19

Why does the melting + boiling points of metals increase from sodium to aluminium?

Answer 19

because of strength of metallic bonding

Question 20

What happens to the charge on the ion as you go from left to right?

Answer 20

charge on ion increases

Question 21

What happens as charge on ion increases as you go from left to right?

Answer 21

so more electrons join delocalised electron ‘sea’ that holds giant metallic lattice together

Question 22

What does the melting point of non-metals with molecular structures depend on?

Answer 22

size of van der Waals forces between molecules

Question 23

As the melting point of non-metals with molecular structures depend on size of VDW forces between molecules, what does this in turn depend on?

Answer 23

number of electrons in molecules + how closely the molecules can pack together

Question 24

Why does silicon have a much higher melting point?

Answer 24

it has a giant structure