2.2.2 - Bonding and Structure

Question 1

Why do elements bond?

Answer 1

To achieve a full outer electron shell.

Question 2

How do atoms bond?

Answer 2

By transferring or sharing electrons.

Question 3

Define ionic bonding.

Answer 3

The electrostatic attraction between positive and negative ions.

Question 4

Define covalent bonding.

Answer 4

The attraction between a shared pair of electrons and the nuclei of bonded atoms.

Question 5

What kind of elements form ionic bonds?

Answer 5

Metals and non-metals.

Question 6

What kind of elements form covalent bonds?

Answer 6

Non-metals.

Question 7

What is a dot and cross diagram used for?

Answer 7

To represent the transfer or sharing of electrons in bonding.

Question 8

What happens when potassium bonds with fluorine?

Answer 8

Potassium gives an electron to fluorine, forming K⁺ and F⁻ ions.

Question 9

What do ionic compounds form?

Answer 9

A giant ionic lattice structure.

Question 10

Why do ionic compounds have high melting points?

Answer 10

Strong electrostatic forces require a lot of energy to break.

Question 11

What increases the melting point of an ionic compound?

Answer 11

Greater charges on the ions.

Question 12

Are ionic compounds soluble in water?

Answer 12

Yes, if the lattice breaks and water attracts the ions.

Question 13

Can solid ionic compounds conduct electricity?

Answer 13

No, because ions are fixed in place.

Question 14

Can molten or aqueous ionic compounds conduct?

Answer 14

Yes, ions are free to move and carry charge.

Question 15

Define metallic bonding.

Answer 15

The attraction between positive metal ions and delocalised electrons.

Question 16

What is a lone pair of electrons?

Answer 16

A pair of valence electrons not involved in bonding.

Question 17

What is a bonding pair?

Answer 17

A pair of electrons shared between atoms in a covalent bond.

Question 18

What is a single covalent bond?

Answer 18

One pair of shared electrons.

Question 19

What is a double covalent bond?

Answer 19

Two shared pairs of electrons.

Question 20

What is a triple covalent bond?

Answer 20

Three shared pairs of electrons.

Question 21

What does “localised” mean in covalent bonding?

Answer 21

The electrons are shared only between the bonded atoms.

Question 22

What is a dative covalent bond?

Answer 22

One atom donates both electrons in the shared pair.

Question 23

What ion does sulfur form?

Answer 23

S²⁻

Question 24

Give an example of a dative bond.

Answer 24

NH₄⁺ (ammonium ion)

Question 25

What ion does sulfate form?

Answer 25

SO₄²⁻

Question 26

What ion does carbonate form?

Answer 26

CO₃²⁻

Question 27

What ion does hydroxide form?

Answer 27

OH⁻

Question 28

What is the formula for magnesium fluoride?

Answer 28

MgF₂

Question 29

What is the formula for barium hydroxide?

Answer 29

Ba(OH)₂

Question 30

True or False: Solid ionic compounds conduct electricity.

Answer 30

False

Question 31

How many bond pairs in N₂?

Answer 31

3 bond pairs, 2 lone pairs.

Question 32

What is the electronic configuration of Cl?

Answer 32

1s² 2s² 2p⁶ 3s² 3p⁵

Question 33

What is the formula of aluminum ion?

Answer 33

Al³⁺

Question 34

What is the formula of hydrogen peroxide?

Answer 34

H₂O₂

Question 35

What’s the term for simultaneous oxidation and reduction?

Answer 35

Redox

Question 36

How many electrons can an orbital hold?

Answer 36

2 electrons

Question 37

What’s the formula for sulfuric acid?

Answer 37

H₂SO₄

Question 38

What does 2n² represent?

Answer 38

Max number of electrons in a shell.

Question 39

What is the maximum number of electrons in the 2nd shell?

Answer 39

8

Question 40

What is an ion?

Answer 40

A charged particle formed by loss or gain of electrons.

Question 41

What holds metallic structures together?

Answer 41

Delocalised electrons and positive metal ions.

Question 42

Are covalent bonds strong or weak?

Answer 42

Strong

Question 43

Why are giant covalent structures like diamond hard?

Answer 43

Many strong covalent bonds throughout the structure.

Question 44

What is the shape of CH₄?

Answer 44

Tetrahedral

Question 45

What is the bond angle in NH₃?

Answer 45

107°

Question 46

What is the bond angle in H₂O?

Answer 46

104.5°

Question 47

What is the bond angle of a linear atom?

Answer 47

180°

Question 48

What is the bond angle of a trigonal planar?

Answer 48

120°

Question 49

What is the bond angle of a tetrahedral

Answer 49

109° or 109.5°

Question 50

What is the bond angle of a triangular bipyramid?

Answer 50

90° and 120°

Question 51

What is the bond angle of an Octahedral?

Answer 51

°

Question 52

How many electron pairs does an Octaherdal shape have?

Answer 52

6

Question 53

How many electron pairs does a Triangular Bipyramid shape have?

Answer 53

5

Question 54

How many electron pairs does a Tetrahedral shape have?

Answer 54

4

Question 55

How many electron pairs does a Trigonal Planar shape have?

Answer 55

3

Question 56

How many electron pairs does a Linear shape have?

Answer 56

2

Question 57

Why do different molecules have different shapes?

Answer 57

Electron Pair Repulsion Theory - The electron pairs surrounding a central atom determine the shape of the molecule or ion - The electron pairs repel one another so that they are arranged as far apart as possible - Different numbers of electron pairs result in different shapes

Question 58

How many Bond Pairs & Lone Pairs does a non-linear shape have?

Answer 58

2 BP, 2 LP

Question 59

How many Bond Pairs & Lone Pairs does a Pyramidal shape have?

Answer 59

3 BP, 1 LP

Question 60

How many Bond Pairs & Lone Pairs does a Tetrahedral shape have?

Answer 60

4 BP, 0 LP

Question 61

What is the bond angle of a non-linear atom?

Answer 61

104.5°

Question 62

What is the bond angle of a Pyramidal atom?

Answer 62

107°

Question 63

What are intermolecular forces?

Answer 63

Forces between molecules that determine the physical properties of molecules like their boiling point, melting point, and density

Question 64

What are the 3 types of Intermolecular forces?

Answer 64

Induced dipole-dipole interaction (London Forces) Permanent dipole – dipole interactions Hydrogen Bonding

Question 65

How do London Forces (Induced dipole - dipole) form?

Answer 65

Uneven distribution of electrons This results in a slightly negative (δ−) and slightly positive (δ+) charge on either side of the atom. A temporary dipole has been established. This temporary dipole induces a temporary dipole on the neighbouring molecule.

Question 66

What is Hydrogen Bonding?

Answer 66

Hydrogen bonding is the intermolecular force that occurs between molecules containing these permanent dipoles. Hydrogen bonding is the strongest type of intermolecular force. There is a large difference in electronegativity between H and O,N,F which results in a strong permanent dipole.

Question 67

Which is denser, Ice or Water?

Answer 67

Water

Question 68

Why is Water more denser than Ice?

Answer 68

Ice has an open lattice structure in which the water molecules are held equally apart When liquid the lattice structure collapses, molecules move closer together making it more dense