Unit1Topic6 - The Periodic Table

Question 1

The Newlands structure of the Periodic Table

Answer 1

• arranged elements in order of increasing atomic mass

- noticed similarities between each 8th element (called the Newlands Octaves)

Question 2

The Mendeleev structure of the Periodic Table

Answer 2

• left gaps for undiscovered elements
• arranged elements in groups and periods
• separated the metals and non-metals
• arranged elements in order of increasing atomic mass

Question 3

How the modern Periodic Table differs from Mendeleev

Answer 3

• no gaps
• noble gases
• elements arranged in order of atomic number
• actinides and lanthanides

Question 4

Name of group 1

Answer 4

Alkali metals

Question 5

Name of group 2

Answer 5

Alkaline earth metals

Question 6

Name of group 7

Answer 6

Halogens

Question 7

Name of group 8

Answer 7

Noble gases

Question 8

Name of block between groups 2 and 3

Answer 8

Transition metals

Question 9

Which elements are the only liquids on the Periodic Table?

Answer 9

Br and Hg

Question 10

Across a period the…

Answer 10

• atoms decrease in size
• elements change from metals to non-metals
• oxides of the elements change from basic to acidic
• semi-metals (properties between metals and non-metals) are found between metals and non-metals e.g. silicon

Question 11

Why do the atoms gradually decrease in size across a period?

Answer 11

The extra electron going into the same shell and the extra positive charge on the nucleus, caused by the extra proton, increases the attraction on the shells pulling them closer to the nucleus.

Question 12

As you go down groups 1 and 2…

Answer 12

• bigger atoms (there is one extra full shell of electrons for each row you go down)
• more reactive (outer electron is more easily lost as further from the nucleus)
• more dense
• even softer to cut
• lower melting point / boiling point

Question 13

Metal + water ->

Answer 13

Metal hydroxide + hydrogen

Question 14

Metal + oxygen ->

Answer 14

Metal oxide

Question 15

Metal + acid ->

Answer 15

Salt + hydrogen

Question 16

Metal + halogen ->

Answer 16

Metal halide

Question 17

Potassium in water observations

Answer 17

• bubbles of gas / fizzes
• moves across surface
• potassium disappears
• catches fire / burns with a lilac flame

Question 18

Why is lithium stored under oil?

Answer 18

It could react with the moisture in the air

Question 19

Why should caesium never be added to water?

Answer 19

It’s highly reactive (explosive)

Question 20

Lithium in water observations

Answer 20

• fizzes
• moves across surface
• sodium disappears
• melts into a ball

Question 21

How would you show the final solution contained potassium hydroxide?

Answer 21

Use Universal indicator, which will turn dark blue

Question 22

Why do all group 1 metals have similar chemical properties?

Answer 22

They all have 1 electron to lose in their outer shell

Question 23

Fluorine (F2) appearance

Answer 23

Pale yellow gas

Question 24

Chlorine (Cl2) appearance

Answer 24

Pale green gas

Question 25

Bromine (Br2) appearance

Answer 25

Red-brown volatile liquid

Question 26

Iodine (I2) appearance

Answer 26

Dark black solid gives purple vapour

Question 27

As you go down group 7…

Answer 27

• bigger atoms
• less reactive
• less soluble (although none of the halogens are very soluble)
• increasing melting point / boiling point
• change of state from gas -> liquid -> solid

Question 28

Physical properties of chlorine

Answer 28

• pale green gas
• heavier (denser than air)
• toxic
• slightly soluble in water
• bleaches damp litmus paper (this is the test for chlorine)

Question 29

Source of chlorine

Answer 29

Electrolysis of sodium chloride (brine)

Question 30

Uses of chlorine

Answer 30

• manufacture of PVC
• bleach
• water sterilisation (used to kill germs in swimming pools and drinking water)

Question 31

Displacement reaction - a …… ………… halogen can displace a …… ………… halogen from a solution of its salt

Answer 31

More reactive

Less reactive

Question 32

Displacement reaction - when chlorine reacts with potassium bromide

Answer 32

Solution turns orange (bromine in water is produced)

Question 33

Displacement reaction - when chlorine reacts with potassium iodide

Answer 33

Solution turns brown (iodine in water is produced)

Question 34

Displacement reaction - when bromine reacts with potassium chloride

Answer 34

Solution remains orange (no reaction)

Question 35

Displacement reaction - when bromine reacts with potassium iodide

Answer 35

Solution turns brown (iodine in water is produced)

Question 36

Displacement reaction - when iodine reacts with potassium chloride

Answer 36

Solution remains brown (no reaction)

Question 37

Displacement reaction - when iodine reacts with potassium bromide

Answer 37

Solution remains brown (no reaction)

Question 38

Physical description of bromine

Answer 38

• liquid

- red-brown

Question 39

Most common use for the noble gases

Answer 39

Neon, glowing signs

Question 40

Colour helium produces as a neon, glowing sign

Answer 40

A pale pink light

Question 41

Properties of all metals

Answer 41

• hard
• shiny
• high melting / boiling points
• malleable and ductile
• sonorous (produce sound when struck)
• conduct heat and electricity
• strong

Question 42

Trends within a group

Answer 42

• have the same number of outer electrons
• similar properties
• atom size increases as you go down a group

Question 43

Metals are found on the …… …… ……, non-metals on the …… …… ……

Answer 43

Metals - left hand side

Non-metals - right hand side

Question 44

Metals form metal oxides which are…

Non-metals form oxides which are…

Some elements in the middle of the table form oxides that show… These are called…

Answer 44

Metals form metal oxides which are basic (remember a soluble base is called an alkali)

Non-metals form oxides which are acidic (e.g. sulfur dioxide SO4)

Some elements in the middle of the table form oxides that show acidic and basic properties (e.g. aluminium oxide). These are called amphoteric oxides.