1.3 - Bonding

Question 1

What is ionic bonding?

Answer 1

Strong, electrostatic forces of attraction between oppositely charged ions held in a lattice

Question 2

Give an example of an ionically bonded substance

Answer 2

NaCl

Question 3

How high are ionically bonded substances, boiling point and melting points? why?

Answer 3

High – takes a lot of energy to break strong, electrostatic forces of attraction between oppositely charged ions

Question 4

Do ionic compounds conduct electricity? why?

Answer 4

Yes, when molten/in solution is the ions are free to move and carry charge

Question 5

What is simple molecular covalent bonding?

Answer 5

Strong covalent bonds between atoms week VanderWaal forces of attraction between molecules

Question 6

Are there any loan electrons in simple covalent bonding?

Answer 6

No, all involved in bonding

Question 7

Can simple molecular covalent molecules conduct electricity?

Answer 7

No, all electrons used in bonding and aren’t free to move

Question 8

Do you simple molecular substances have high/low, melting points, or boiling points?

Answer 8

No – week, VanderWaal forces of attraction between molecules that don’t take much energy to overcome

Question 9

Describe, macromolecular, covalent bonding

Answer 9

Lattice of many atoms held together by strong covalent bonds

Question 10

Do substances with macromolecular covalent bonds have high/low, melting point and boiling points?

Answer 10

High, as it takes a lot of energy to overcome many strong covalent bonds

Question 11

Do you substances with macromolecular, covalent bonds, conduct, electricity?

Answer 11

Most don’t is all electrons are used in bonding 

Question 12

Describe the structure of diamond

Answer 12

3-D. Tetrahedral structure of C atoms with each C atom bonded to 4 others.

Question 13

Describe the structure of graphite

Answer 13

Similar to diamond macromolecular covalent, but each see atom is only bonded to 3 others, so it is in layers.

Wake VanderWaal forces of attraction between layers mean, they can slide over each other – soft, slippery

One electron from each carbon is delocalised and can carry charge – conducts, electricity

Question 14

Describe metallic bonding

Answer 14

Lattice of positive metal ions strongly attracted to receive delocalised electrons. Latest can slide over each other - malleable.

Question 15

Do metallic compounds have high/low boiling point than melting points?

Answer 15

High – a strong forces of attraction between positive metal ions and negatively charged, see if delocalised electrons

Question 16

Do metallic compounds conduct, electricity?

Answer 16

Yes, as delocalised electrons can move throughout the metal to carry charge

Question 17

How does the strength of metallic bonds change cross the periodic table?

Answer 17

It increases high, melting and boiling points, stronger higher charges on metal ions

More delocalised electrons per ion

Stronger forces of attraction between them

Question 18

Define electronegativity

Answer 18

The ability of an atom to attract a pair of electrons in a covalent bond

Question 19

What affects electronegativity?

Answer 19

Nuclear charge
Atomic radius
Electron shielding

Question 20

What are the four most electronegative elements?

Answer 20

Fluorine
Oxygen
nitrogen
Chlorine

Question 21

How do you get a nonpolar bond?

Answer 21

Both bonding elements have the same electronegativities

Question 22

When do you get a polar bond?

Answer 22

Bonding atoms have different electronegativities

Question 23

What is the strongest type of intermolecular force?

Answer 23

Hydrogen bonding

Question 24

What is the weakest type of intermolecular force?

Answer 24

Vander Waals

Question 25

Describe VanderWaals, forces of attraction

Answer 25

Temporary dipoles created by the random movement of electrons Induced dipole in neighbouring molecules Temporary induced dipole, dipole attraction, a.k.a. Vandivers force of attraction

Question 26

Are VanderWaal forces stronger in smaller or larger molecules?

Answer 26

Larger – more electrons

Question 27

Describe permanent, dipole-dipole attraction

Answer 27

Some molecules with polar bonds have permanent dipoles Forces of attraction between those dipoles and those of neighbouring molecules

Question 28

Why is ice less dense than liquid water?

Answer 28

In liquid water, hydrogen bonds, constantly breaking reform as molecules move around In ice, the hydrogen bonds hold the molecules in fixed positions. This makes them slightly further apart than liquid water.

Question 29

What is a dative covalent bond?

Answer 29

Formed when an electron deficient atom, except the lone pair of electrons from an atom with a lone pair of electrons

Question 30

What does the shape of molecules depend on?

Answer 30

Number of electrons in the valance shell of the central atom Number of these electrons which are in bonded a lone pairs

Question 31

What does electron pair repulsion theory state?

Answer 31

That electron pairs will take up positions as far away from each other as possible to minimise the opposing forces between them

Question 32

2 bonded pairs, 0 lone pairs

Answer 32

Linear 180°

Question 33

3 BP, 0LP

Answer 33

Trigonal planar 120°

Question 34

4BP, 0LP

Answer 34

Tetrahedral 109.5°

Question 35

5BP, 0LP

Answer 35

Trigonal bipyramidal 90° and 120°

Question 36

6BP, 0LP

Answer 36

Octahedral 90°