Chem (26.1.23)

Question 1

What are ions?

Answer 1

-> charged atoms or molecules
-can be single atoms (eg. Na +), or a group of atoms (eg. NO3 -)

Question 2

What are Cations?

Answer 2

+ ions, formed by gaining electrons, metal
-single atoms which have lost either 1,2 or 3 electrons to achieve a FULL outer shell, molecules with a net POSITIVE CHARGE

Question 3

What are Anions?

Answer 3

-ions, formed by losing electrons, non-metal
-single atoms which have gained either 1,2 or 3 electrons to achieve a FULL outer shell, molecules with a net NEGATIVE CHARGE

Question 4

What do ions in Group 1 form?

Answer 4

1+ ions

Question 5

What do ions in Group 2 form?

Answer 5

2+ ions

Question 6

What do ions in Group 3 form?

Answer 6

3+ ions

Question 7

What do ions in Group 5 form?

Answer 7

3- ions

Question 8

What do ions in Group 6 form?

Answer 8

2- ions

Question 9

What do ions in Group 7 form?

Answer 9

1- ions

Question 10

What is the Sulphate ion?

Answer 10

SO4 2- (2-goes on top)

Question 11

What is the Carbonate ion?

Answer 11

CO3 2- (2-goes on top)

Question 12

What is the Nitrogen ion?

Answer 12

NO3 - (- goes on top)

Question 13

What is the Hydroxide ion?

Answer 13

OH - (- goes on top)

Question 14

What is the Ammonium ion?

Answer 14

NH4 + (+ goes on top)

Question 15

What is the Silver ion?

Answer 15

Ag + (+ goes on top)

Question 16

What is the Zinc ion?

Answer 16

Zn 2+ (2+ goes on top)

Question 17

What is the Copper ion?

Answer 17

Cu 2+ (2+ goes on top)

Question 18

What is the Lead (II) ion?

Answer 18

Pb 2+ (2+ goes on top)

Question 19

What is the Hydrogen ion?

Answer 19

H + (+ goes on top)

Question 20

What is the Iron (II) ion?

Answer 20

Fe 2+ (2+ goes on top)

Question 21

What is the Iron (III) ion?

Answer 21

Fe 3+ (3+ goes on top)

Question 22

What is the Giant Ionic Lattice Structure?

Answer 22

-ionic compounds have a giant ionic lattice structure
-made of millions of oppositely charged ions, their formula is the simplest ratio of the ions (ie. the empirical formula)
-the higher the charge, the stronger the attraction

Question 23

What are some properties of Ionic Compounds?

Answer 23

-high melting/boiling points -> millions of strong bonds need to be broken
-don’t conduct electricity -> electrons are not free to move through the solid
-conduct electricity in molten and in aqueous solution -> ions are free to move
-dissolve in water-> able to form strong electrostatic attraction with the ions
-HARD -> due to strong forces between the ions

Question 24

What are the Properties of Non-Metals on the Periodic Table?

Answer 24

-poor conductors of electricity
-non-metal oxides are acidic -> form solutions with a pH less than 7

Question 25

What are the Properties of Metals on the Periodic Table?

Answer 25

-conduct electricity
-metal oxides are basic-> form solutions with a pH more than 7

Question 26

How can you use the positions of two elements to predict the n. of electrons they will gain when they form ions? (Sulphur + Chlorine)

Answer 26

-the n. of electrons gained is equal to 8- the group number.
Sulfur is in Group 6, 8-6 = 2 electrons gained, Chlorine is in Group 7, 8-7= 1 electron gained

Question 27

Why can’t Nitrate ions and Bromine ions form ionic compounds?

Answer 27

-They are both negatively charged -> ionic compounds can only be formed between negative and positive ions

Question 28

In the periodic table, what do electronic configurations of elements in the same group have in common?

Answer 28

-they have the same n. of electrons in their outer shell