Bonding

Question 1

Define an ionic bond

Answer 1

The electrostatic force of attraction between oppositely charged ions formed by electron transfer

Question 2

Define covalent bond

Answer 2

A shared pair of electrons

Question 3

Define a dative covalent bond

Answer 3

The shared pair of electrons in the covalent bond come from only one of the bonding atoms

Question 4

Define a metallic bond

Answer 4

The electrostatic force of attraction between the positive metal ions and the delocalised electrons

Question 5

What are the 3 factors which affect the strength of a metallic bond and state which ones lead to a stronger metallic bond?

Answer 5

Number of protons (more=stronger bond)
Number of delocalised electrons per atom (more=stronger bond)
Size of atom (smaller=stronger bond),

Question 6

What are 4 examples of macromolecular covalent structures?

Answer 6

Diamond
Graphite
Silicon Dioxide
Silicon

Question 7

What’s the solubility like of ionic compounds in water?

Answer 7

Good

Question 8

What’s the solubility like of simple molecular compounds in water?

Answer 8

Poor

Question 9

What’s the conductivity like of ionic compounds when solid, and why?

Answer 9

Poor as Ions can’t moved

Question 10

What’s the conductivity like of ionic compounds when molten, and why?

Answer 10

Good as ions can move

Question 11

What’s the name and bond angle of the shape with 4 bonding pairs and 0 lone pairs

Answer 11

Tetrahedral and 109.5°

Question 12

What’s the name and bond angle of the shape with 3 bonding pairs and 1 lone pairs

Answer 12

Trigonal Pyramidal and 107°

Question 13

What’s the name and bond angle of the shape with 2 bonding pairs and 2 lone pairs

Answer 13

Bent and 104.5°

Question 14

What’s the name and bond angle of the shape with 5 bonding pairs and 0 lone pairs

Answer 14

Trigonal Bipyramidal and 120° and 90°

Question 15

What’s the name and bond angle of the shape with 6 bonding pairs and 0 lone pairs

Answer 15

Octahedral and 90°

Question 16

Define electronegativity

Answer 16

Relative tendency of an atom in a covalent bond in a molecule to attract electrons in a covalent bond to itself

Question 17

What is the scale where electronegativity is measured in?

Answer 17

Paulin Scale

Question 18

What factors affect electronegativity?

Answer 18

Number of protons
Electron shielding
Distance from the nucleus (atomic radius)

Question 19

What is the most electronegative element?

Answer 19

Fluorine

Question 20

What value does the most electronegative element have on the electronegativity scale?

Answer 20

4.0

Question 21

Why is CCl4 non-polar whilst CH3Cl polar?

Answer 21

CH3Cl is asymmetrical due to the presence of C-Cl bond which is polar

Question 22

In polar covalent bonds what slight charge does carbon and hydrogen atoms tend to have?

Answer 22

Delta Positive

Question 23

What makes a compound purely covalent?

Answer 23

Small electronegative difference between elements

Question 24

What makes a compound mostly ionic?

Answer 24

Large electronegative difference between elements

Question 25

What is the relationship between symmetry and polarity

Answer 25

Symmetrical are non-polar

Question 26

Which substances show van der waals forces?

Answer 26

Molecular compounds

Question 27

Which substances do not show van der waals forces?

Answer 27

Ionic compounds

Question 28

When do permanent dipole-dipole forces occur?

Answer 28

When there is a difference in electronegativity between elements/elements that are polar

Question 29

When does hydrogen bonding occur and what must be present?

Answer 29

Between hydrogen and either fluorine, oxygen and nitrogen. There must be also be a lone-pair of electrons.

Question 30

Why does H2O, NH3 and HF all have anomalously high boiling points?

Answer 30

They all show hydrogen bonding