AI Group 1 and 7

Question 1

What is the relationship between electron loss and metal reactivity?

Answer 1

The easier it is to lose the electron, the more reactive the metal.

Question 2

Which group is more reactive: group 1 or group 7?

Answer 2

Group 1 will be more reactive than group 7.

Question 3

Why is group 1 more reactive than group 7?

Answer 3

It is easier to lose 1 electron than 2.

Question 4

How does reactivity change as you go down group 7?

Answer 4

As you go down group 7, the reactivity decreases.

Question 5

What test is used to react with chlorides, bromides, and iodides?

Answer 5

The silver nitrate test.

Question 6

What is the first step in the silver nitrate test?

Answer 6

Nitric acid is first added to the solution to be tested.

Question 7

What is the second step in the silver nitrate test?

Answer 7

Three drops of silver nitrate solution are then added to the solution.

Question 8

What group do halogens belong to?

Answer 8

Group 7.

Question 9

True or False: The harder it is to lose an electron, the more reactive the metal.

Answer 9

False

Question 10

What group of the periodic table do the halogens belong to?

Answer 10

Group VII

Question 11

What characteristic do all halogens share regarding their molecular structure?

Answer 11

They are diatomic

Question 12

What is the state of chlorine at room temperature?

Answer 12

Gas

Question 13

What color is chlorine in its raw form?

Answer 13

Pale green

Question 14

What are two uses of chlorine?

Answer 14

• Make bleaches
• Treat public drinking water

Question 15

What is the state of bromine at room temperature?

Answer 15

Liquid

Question 16

What color is bromine?

Answer 16

Red-brown

Question 17

What is one use of bromine?

Answer 17

Used by gardeners in pesticides

Question 18

What is the state of iodine at room temperature?

Answer 18

Solid

Question 19

What color is iodine?

Answer 19

Grey

Question 20

What is one use of iodine?

Answer 20

Used as an antiseptic on wounds

Question 21

What happens when hot sodium reacts with chlorine?

Answer 21

There is a bright yellow glow and sodium chloride is formed

Question 22

What is the chemical formula for sodium chloride?

Answer 22

NaCl

Question 23

Fill in the blank: Lithium + bromine → _______.

Answer 23

Lithium Bromide

Question 24

What is the chemical equation for lithium reacting with bromine?

Answer 24

2 Li + Br2 → 2 LiBr

Question 25

What must be done when handling halogens in a school?

Answer 25

Handle very carefully and use in a fume cupboard

Question 26

Are halogens toxic?

Answer 26

True

Question 28

What happens to the reactivity of halogens as you go down the group?

Answer 28

Reactivity decreases as you go down the group ## Footnote This is due to the increasing atomic size and decreased attraction of the outer electrons.

Question 29

Which elements in Group 7 are mentioned?

Answer 29

Fluorine and Chlorine ## Footnote Fluorine has an atomic number of 9, and Chlorine has an atomic number of 17.

Question 30

What is the electronic configuration of Fluorine?

Answer 30

2, 7 ## Footnote Fluorine has 2 electrons in the first shell and 7 in the second.

Question 31

What is the electronic configuration of Chlorine?

Answer 31

2, 8, 7 ## Footnote Chlorine has 2 electrons in the first shell, 8 in the second, and 7 in the third.

Question 32

How do halogens react with sodium and iron?

Answer 32

They react vigorously ## Footnote The nature of the reaction varies as you move down the group.

Question 33

Fill in the blank: The halogens react by _______ an electron.

Answer 33

gaining

Question 34

What trend is observed in atomic size as you go down Group 7?

Answer 34

Atomic size increases ## Footnote Larger atomic size results in decreased attraction of outer electrons.

Question 35

True or False: The reactivity of Group 6 elements is expected to be greater than that of Group 7 elements.

Answer 35

False

Question 36

What factors contribute to the decreased reactivity of halogens as you descend the group?

Answer 36

Increased atomic size and decreased attraction of outer electrons ## Footnote The outer electrons are further from the nucleus, making it harder to attract additional electrons.