Ionic Bonding

Question 1

What is an ion?

Answer 1

An ion is an electrically charged atom or group of atoms formed by the loss or gain of electrons.

Question 2

Why do atoms lose and gain electrons?

Answer 2

This loss or gain of electrons takes place to obtain a full outer shell of electrons.

Question 3

The electronic structure of ions of elements in groups 1, 2, 3, 5, 6 and 7 will be the same as which has?

Answer 3

The electronic structure of ions of elements in groups 1, 2, 3, 5, 6 and 7 will be the same as that of a noble gas - such as helium, neon, and argon.

Question 4

What are negative ions and when are they formed?

Answer 4

Negative ions are called anions and form when atoms gain electrons, meaning they have more electrons than protons

Question 5

What are anions and when are they formed?

Answer 5

Anions are Negative ions and are formed when atoms gain electrons, meaning they have more electrons than protons

Question 6

What are positive ions called and when are they formed?

Answer 6

Positive ions are called cations and form when atoms lose electrons, meaning they have more protons than electrons.

Question 7

What are cations and when are they formed?

Answer 7

Cations are Positive ions and form when atoms lose electrons, meaning they have more protons than electrons

Question 8

All metals lose electrons to become what?

Answer 8

All metals lose electrons to other atoms to become positively charged ions

Question 9

All non-metals lose or gain electrons and why?

Answer 9

All non-metals gain electrons from other atoms to become negatively charged ions.

Question 10

How to deduce the charge of an ion?

Answer 10

Find the number of electrons in the outer electron shell
Find out if it is easy for the atom to gain electron or to donate electron (in most cases atoms that have fewer than four electrons, donate electrons and atoms that have more than 4 electrons, receive electrons)
Atoms that gain electrons become negative ions and atoms that donate electron forms positive ion.

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Question 11

Charge/Formula of Group 1 Metals (Li, Na, K, Rb, Cs, Fr)

Answer 11

1+

Question 12

Charge/Formula of Group 2 Metals (Be, Mg, Ca, Sr, Ba, Ra)

Answer 12

2+

Question 13

Charge/Formula of Group 3 Metals (Al, Ga, In, Ti)

Answer 13

3+

Question 14

Charge/formula of silver

Answer 14

Ag+

Question 15

Charge/formula of Copper (II)

Answer 15

Cu 2+

Question 16

Charge/formula of Iron (II)

Answer 16

Fe2+

Question 17

Charge/formula of Iron (III)

Answer 17

Fe 3+

Question 18

Charge/formula of Lead

Answer 18

Pb 2+

Question 19

Charge/formula of Zinc

Answer 19

Zn 2+

Question 20

Charge/formula of Hydrogen

Answer 20

H+

Question 21

Charge/formula of Ammonium

Answer 21

NH4 +

Question 22

Charge/formula of Group 5 Non-Metals (N, P, As)

Answer 22

3-

Question 23

Charge/formula of Group 6 Non-Metals (O, S, Se)

Answer 23

2-

Question 24

Charge/formula of Group 7 Non-Metals (F, Cl, Br, I, At)

Answer 24

1-

Question 25

Charge/formula of Hydroxide

Answer 25

OH-

Question 26

Charge/formula of Carbonate

Answer 26

CO3 2-

Question 27

Charge/formula of Nitrate

Answer 27

NO3 -

Question 28

Charge/formula of Sulfate

Answer 28

SO4 2-

Question 29

Formula and charge of Chromium (III)

Answer 29

Cr3+

Question 30

Formula and charge of Ammonium

Answer 30

NH4 +

Question 31

Formula and Charge of Hydrogen Carbonate

Answer 31

HCO3 -

Question 32

How are ionic compounds held together?

Answer 32

The positive and negative charges are held together by the strong electrostatic forces of attraction between oppositely charged ions.

Question 33

Ionic compounds are made of charged particles called ions which form a…

Answer 33

Ionic compounds are made of charged particles called ions which form a giant lattice structure.

Question 34

Explain the melting and boiling points of ionic substances

Answer 34

Ionic substances have high melting and boiling points due to the presence of strong electrostatic forces acting between the oppositely charged ions
These forces act in all directions and a lot of energy is required to overcome them.

Question 35

Describe the state of ionic compounds at room temperature

Answer 35

Ionic compounds are usually solid at room temperature and are non-volatile (do not vaporise easily)

Question 36

Why do ionic substances tend to be soluble in water?

Answer 36

Ionic substances tend to be soluble in water as both ionic compounds and water are polar ( contains a region of partial positive and negative charge)substances

Question 37

Ions with a higher charge will have what?

Answer 37

Ions with higher charge have stronger electrostatic forces and will thus have higher melting and boiling points.

Question 38

For electrical current to flow in ionic compounds what must must there be present?

Answer 38

For electrical current to flow there must be present freely moving charged particles such as electrons or ions

Question 39

Explain if ionic compounds can conduct electricity

Answer 39

Ionic compounds can conduct electricity in the molten state or in solution as they have ions that can move and carry charge
They cannot conduct electricity in the solid state as the ions are in fixed positions within the lattice and are unable to move