periodic table

Question 1

definition of diatomic elements

Answer 1

two atoms of the same element covalently bonded together

Question 2

7 diatomic elements

Answer 2

H (hydrogen), Nitrogen (N), Fluorine (F), Oxygen (O), Iodine (I), Chlorine (Cl), Bromine (Br)

Question 3

how is the periodic table arranged

Answer 3

• in order of atomic number
• in groups and periods

Question 4

ways to identify whether its a metal or non-metal

Answer 4

• electrical conductivity
• acid-base character of bases

Question 5

can metal conduct electricity

Answer 5

yes

Question 6

can non-metals conduct electricity

Answer 6

no

Question 7

is metal oxides acidic or alkaline

Answer 7

alkaline

Question 8

is non-metal oxides acidic or alkaline

Answer 8

acidic

Question 9

why do elements in the same group have similar chemical properties

Answer 9

they have the same number of electrons in their outer shell

Question 10

why are noble gases unreactive

Answer 10

they have a full valence shell, they don’t need to gain or loose any electrons

Question 11

features of the alkali metals

Answer 11

• most reactive metals
• reacts with water to produce a hydroxide
• less dense than water (float on surface)
• have relatively low melting point

Question 12

what does the reaction of alkali metals and water produce

Answer 12

• hydroxide solution
• hydrogen

Question 13

how does lithium react with water

Answer 13

• vigorously
• fizzing
• effervescence
• moves on the surface of water
• piece of metal gets smaller

Question 14

equation for the reaction of lithium and water

Answer 14

lithium + water -> lithium hydroxide + hydrogen
2Li(s) + 2H2O(l) -> 2LiOH(aq) + H2(g)

Question 15

how does sodium react with water

Answer 15

• vigorously
• fizzing
• effervescence
• moves on the surface of water
• piece of metal gets smaller
• reacts more rapidly than lithium

Question 16

equation for the reaction of sodium and water

Answer 16

sodium + water -> sodium hydroxide + hydrogen
2Na(s) + 2H2O(l) -> 2NaOH(aq) + H2(g)

Question 17

how does potassium react with water

Answer 17

• vigorously
• fizzing
• effervescence
• moves on the surface of water
• piece of metal gets smaller
• purple flame

Question 18

what does the reaction of lithium and oxygen produce

Answer 18

lithium oxide (Li2O)

Question 19

what does the reaction of sodium oxygen produce

Answer 19

sodium oxide (Na2O) or sodium peroxide (Na2O2)

Question 20

what does the reaction of potassium and oxygen produce

Answer 20

potassium peroxide (K2O2) or potassium superoxide (KO2)

Question 21

what is the reactivity trend in group 1 metals

Answer 21

the metal becomes more reactive as you go down the group

Question 22

explain the reactivity trend in group 1 metals

Answer 22

when the atom becomes bigger, the atomic radius increases. Thus, the outer electron becomes further from the nucleus which decreases the force of attraction between the nucleus and the valence electron. so the electron is lost more easily.

Question 23

examples of alkali metals

Answer 23

• lithium, Li
• Sodium, Na
• Potassium, K
• Rubidium, Rb
• Caesium, Cs
• Francium, Fr

Question 24

physical properties of halogens

Answer 24

• non metals
• highly reactive
• diatomic

Question 25

examples of halogens

Answer 25

- Fluorine, F - Chlorine, Cl - Bromine, Br - Iodine, I - Astatine, At

Question 26

colour and state at room temperature of Fluorine

Answer 26

- Gas - pale yellow

Question 27

colour and state at room temperature of Chlorine

Answer 27

- Gas - pale green

Question 28

colour and state at room temperature of bromine

Answer 28

- liquid - brown

Question 29

colour and state at room temperature of Iodine

Answer 29

- solid - grey

Question 30

vapour colour of Fluorine

Answer 30

pale yellow

Question 31

vapour colour of chlorine

Answer 31

pale green

Question 32

vapour colour of bromine

Answer 32

orange

Question 33

vapour colour of iodine

Answer 33

purple

Question 34

colour of aqueous solution of chlorine

Answer 34

pale green

Question 35

colour of aqueous solution of bromine

Answer 35

orange

Question 36

colour of aqueous solution of iodine

Answer 36

brown

Question 37

the melting point increases down or up the group 7

Answer 37

down

Question 38

the reactivity increases down or up the group 7

Answer 38

up

Question 39

explain the reactivity of halogens

Answer 39

atomic radius decreases as you go up the group, causing a stronger attraction between the nucleus and the valence electron. there it is easier for the halogen to attract an element. therefore reactivity increases as you go up the group

Question 40

explain the halogen displacement reactions

Answer 40

a more reactive halogen can displace a less reactive halogen

Question 41

what happens when you add chlorine water, Cl2 (aq) to potassium chlorine solution, KCl(aq)

Answer 41

no reaction

Question 42

what happens when you add chlorine water, Cl2 (aq) to potassium bromide solution KBr (aq)

Answer 42

Cl2 (aq) + 2KBr (aq) ->2KCl(aq) + Br2 (aq) solution changes from colourless to orange

Question 43

what happens when you add chlorine water, Cl2 (aq) to potassium Iodide solution, KI(aq)

Answer 43

Cl2(aq) + 2I(aq) -> 2Cl (aq) + I2 (aq) solution changes from colourless to brown

Question 44

what happens when you add bromine water, Br2 (aq) to potassium chloride solution, KCl (aq)

Answer 44

no reaction

Question 45

what happens when you add bromine water, Br2 (aq) to potassium bromide solution, KBr (aq)

Answer 45

no reaction

Question 46

what happens when you add bromine water, Br2 (aq) to potassium iodide solution, KI (aq)

Answer 46

Br2 (aq) + 2KI (aq) -> 2KBr (aq) + I2 (aq) solution changes from colourless to orange

Question 47

what happens when you add iodine water, I2 (aq) into potassium chloride solution, KCl (aq)

Answer 47

no reaction

Question 48

what happens when you add iodine water, I2 (aq) into potassium bromide solution, KBr (aq)

Answer 48

no reaction