Group 2

Question 1

Define alkaline earth metals.

Answer 1

Elements in Group 2 of the periodic table, including beryllium, magnesium, and calcium.

Question 2

True or false: Beryllium is the lightest alkaline earth metal.

Answer 2

TRUE

Question 3

Fill in the blank: Magnesium burns with a _______ flame.

Answer 3

bright white

Question 4

What is the general oxidation state of alkaline earth metals?

Answer 4

They typically have an oxidation state of +2.

Question 5

what happens to reactivity in alkaline earth metals.

Answer 5

Reactivity increases down the group, with barium being more reactive than beryllium.

Question 6

What is the trend in melting points of alkaline earth metals?

Answer 6

Melting points generally decrease down the group.

Question 7

Fill in the blank: Strontium is used in _______ fireworks.

Answer 7

red

Question 8

What happens when alkaline earth metals react with water?

Answer 8

They produce hydrogen gas and a metal hydroxide.

Question 9

Define alkaline earth metal hydroxides.

Answer 9

They are strong bases, soluble in water, forming alkaline solutions.

Question 10

What is the effect of heat on alkaline earth metal carbonates?

Answer 10

They decompose to form metal oxides and carbon dioxide.

Question 11

True or false: Radium is radioactive.

Answer 11

TRUE

Question 12

What is the flame test color for strontium?

Answer 12

Crimson red

Question 13

Define alkaline earth metal salts.

Answer 13

Compounds formed from alkaline earth metals and acids, often soluble.

Question 14

Define ionization energy in alkaline earth metals.

Answer 14

The energy required to remove an electron, decreases down the group.

Question 15

What is the density trend in alkaline earth metals?

Answer 15

Density generally increases down the group.

Question 16

True or false: Magnesium can be used to create alloys.

Answer 16

TRUE

Question 17

What is the reaction of alkaline earth metals with halogens?

Answer 17

They form ionic halides.

Question 18

trend in electronegativity in alkaline earth metals.

Answer 18

Electronegativity increases up the group, with beryllium being the lowest.

Question 19

What is the solubility trend of alkaline earth metal hydroxides?

Answer 19

Solubility increases down the group.

Question 20

True or false: Barium is used in X-ray imaging.

Answer 20

TRUE

Question 21

Trends in solubility of group 2 hydroxides

Answer 21

As you go down the group the solubility increases, resulting in the alkalinity of the solution to increase

Question 22

Trends in solubility of group 2 sulfates

Answer 22

solubility decreases down the group

Question 23

Fill in the blank: Barium burns with a _______ flame.

Answer 23

green flame

Question 24

Fill in the blank: Calcium burns with a _______ flame.

Answer 24

red flame

Question 25

the thermal stability of group 2 carbonates & nitrates _____ down the group

Answer 25

increase (as more heat is needed to break them down)

Question 26

Thermal decomposition of group 2 Carbonates

Answer 26

when heated form metal oxides and give off carbon dioxide gas

Question 27

Thermal decomposition of group 2 Nitrates

Answer 27

when heated form metal oxide, nitrogen dioxide and oxygen gas

Question 28

Group 2 carbonates' solubility

Answer 28

all are insoluble in water expect for BeCO3

Question 29

Group 2 carbonates' reaction with HCl & H2SO4

Answer 29

They form soluble chloride salts, water & carbon dioxide with HCl. they form sulfate salts instead of chloride salts With H2SO4

Question 30

Group 2 metal hydroxides react with dilute acids to form _______ solutions of chlorides/sulfate salts | OBSERVATION

Answer 30

colourless

Question 31

Group 2 metals react with dilute acids to form ______ solutions of metal salts | OBSERVATION

Answer 31

colourless

Question 32

What **type of solution** does Group 2 oxides react with water to form?

Answer 32

Alkaline solutions

Question 33

T o F: smaller grp 2 ions have a greater polarising effect on neighbouring negative ions

Answer 33

TRUE

Question 34

What happens to the ΔHlattꝋ of the ionic compounds going down the group?

Answer 34

it decreases as the positively charged cations become bigger meaning more space between the negative & positive ions meaning weaker intermolecular forces

Question 35

What happens to the ΔHhydꝋ going down the group?

Answer 35

also decreases as the ion-dipole bonds between ions & water weaken

Question 36

T or F: The more exothermic the ΔHsolꝋ the less soluble the compound

Answer 36

FALSE

Question 37

what happens to the thermal stability of group 2 nitrates down the group?

Answer 37

increases down the group as the metal cation becomes larger resulting in lower charge density and polarising power meaning more energy is required to break them down

Question 38

What is meant by polarising power?

Answer 38

the ability of a cation to distort or deform the electron cloud of an adjacent anion