CC13- Groups In The Periodic Table

Question 1

What is the electronic configuration of the group 1 metals?

Answer 1

• the alkali metals have one outer electron that they lose to become a 1+ ion
• they all have similar chemical properties since they have the same configuration

Question 2

What are some physical properties of the group 1 alkali metals?

Answer 2

• low melting and boiling points
• very soft and can be cut with a knife

Question 3

What are the reactivity levels like of a group 1 alkali metal and why is it like this?

Answer 3

• alkali metals are very reactive
• they will easily lose their outer electron to create a stable, full outer shell
• reactivity increases going down the group because he outer electron becomes easier to lose
• due to its forces of attraction with the nucleus decreasing as it gets further away with more shells, increasing the distance
• since it’s less strongly attracted to the nucleus, less energy is required to lose it

Question 4

What happens when alkali metals are put into water?

Answer 4

• they react extremely vigorously
• produces a hydroxide of the metal and hydrogen gas
• since reactivity increases going down the group the reaction in water becomes more violent

Question 5

How does lithium react with water?

Answer 5

• bubbles fiercely on the surface, moving around

Question 6

How does sodium react with water?

Answer 6

• Melts into a ball and fizzes on the surface

Question 7

How does potassium react with water?

Answer 7

• melts and then bursts into flames
• flies around on the surface

Question 8

What is the electronic configuration of the group 7 halogens?

Answer 8

• 7 electrons in the outer shell so they all have similar chemical properties
• also all diatomic molecules so they share a pair of electrons in a covalent bond

Question 9

What are some properties of the group 7 halogens?

Answer 9

• non-metallic so they are poor conductors of heat and electricity

Question 10

What is reactivity like in group 7?

Answer 10

• as you go down group seven the melting and boiling points increase, but the reactivity decreases
• this is because it has 7 electrons on the outer shell so they only need to gain 1 in order to have a full outer shell
• when the outer shells are closer to the nucleus it is easier to attract this electron and therefore is more reactive
• going down the group however more electron shells are needed therefore it gets harder for the outer shell to attract another electron since it is further away from the nucleus

Question 11

What is chlorines state like?

Answer 11

• poisonous green gas

Question 12

What is bromines state like?

Answer 12

• poisonous red, brown liquid

Question 13

What is iodines state like?

Answer 13

• purple/black solid

Question 14

How do halogens react with metals?

Answer 14

• they react vigorously to form salts called halides
• halogens higher up in the group will react more since they have less shells, therefore closer to the nucleus and able to attract the extra electron needed for an outer shell

Question 15

How do halogens react with hydrogen?

Answer 15

• creates hydrogen halides
• these are soluble and dissolve in water to create acidic solutions

Question 16

What is the test for chlorine?

Answer 16

• hold damp blue litmus paper over the substance
• if chlorine is present it will turn red, then bleached white
• if there is no change there is no chlorine present

Question 17

What is a halogen displacement reaction like?

Answer 17

• a more reactive halogen can displace a less reactive halogen
• they are redox reactions because the halogen gains electrons (is reduced) and the halides lose them (oxidised) at the same time
• halogens displace the halide ions from its salt

Question 18

How do you test this halogen displacement?

Answer 18

• mix together a halide salt solution and halogen
• shake gently and see if there has been a colour change
• if there has been a colour change a reaction has occurred and the halogen was more reactive than the halide and could displace it

Question 19

What is the electronic configuration of a group 0 noble gas like?

Answer 19

• they are have a full outer shell of electrons and are therefore very stable and won’t easily lose or gain any electrons
• because they have a full outer shell they are INERT and unreactive

Question 20

What are some properties of the group 0 noble gases?

Answer 20

• colourless
• low melting and boiling points
• poor conductors of heat and electricity
• inert (unreactive)
• because they are inert they are also non flammable
• monatomic, made up of single bonds since they do not form bonds with other atoms easily

Question 21

What are some trends in the properties of the noble gases?

Answer 21

• boiling point, melting point and density all increase going down the group

Question 22

What are the main uses for noble gas?

Answer 22

• argon is used in filament lamps since they create an inert, non flammable atmosphere stopping the filament from burning away
• flash photography also uses this same principle with argon, krypton and xenon to stop the flash from burning up
• argon is denser than air so can be used in the space between wine and wine barrels, stopping oxygen from reacting with the wine
• helium on the other hand is less dense than air so it allows aircraft’s and balloons to float