Bonding & Structure (Chapter 5-6)

Question 1

When are ions formed?

Answer 1

When electrons are transferred from one atom to another to gain a full outer shell of electrons

Question 2

What does electrostatic attraction do?

Answer 2

Hold positive and negative ions together

Question 3

What is an ionic bond?

Answer 3

An electrostatic attraction between two oppositely charged ions

Question 4

Why do ionic structures only conduct electricity when molten?

Answer 4

The ions are mobile and can carry the charge

Question 5

Why do ionic compounds have high melting and boiling points?

Answer 5

Giant ionic lattice is held together by strong electrostatic forces. Takes loads of energy to overcome these forces

Question 6

Why can ionic compounds dissolve in water?

Answer 6

Water is polar. So can attract to the different ions lol

Question 7

How many electrons in s sub shell?

Answer 7

2

Question 8

How many electrons in a p sub shell?

Answer 8

6

Question 9

How electrons in a d sub shell?

Answer 9

10

Question 10

How many electrons in a f sub shell?

Answer 10

14

Question 11

What is in the first shell LOL?

Answer 11

1s

Question 12

What is in the second shell?

Answer 12

2s, 2p

Question 13

What is in the third shell?

Answer 13

3s, 3p, 3d

Question 14

What is in the fourth shell?

Answer 14

4s, 4p, 4d, 4f

Question 15

What is the shape of an s orbital?

Answer 15

Circular

Question 16

What is the shape of a p orbital?

Answer 16

Dung bell

Question 17

What is an orbital?

Answer 17

An area of space about the nucleus that can hold a maximum of two electrons with opposite spins

Question 18

What do the Nobel gas symbols mean? Eg. Calcium?

Answer 18

Another way to write electron configuration

Eg. Ca 1s2, 2s2, 2p6, 3s2, 3p6, 4s2
Can also be written as [Ar] 4s2

Question 19

What is a covalent bond?

Answer 19

A covalent bond is the strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

Question 20

Can there be triple and double covalent bonds?

Answer 20

Yes babe

Share 4 or even 6 electrons

Question 21

What can a dative covalent bond be called also?

Answer 21

Coordinate bonding

Question 22

What is a dative bond?

Answer 22

A covalent bond in which both electrons come from the same atom.

Represented with an arrow babe

Question 23

What does the shape of an atom depend on?

Answer 23

The number of pairs of electrons in the outer shell of the central atom

Question 24

What is a lone pair?

Answer 24

Unshared pair of electrons

Question 25

Do electrons repel each other?

Answer 25

Yes- lone pairs repel more than bonding pairs

Question 26

Put this in order of angles biggest to smallest Lone pair/ lone pair Bonding pair/ bonding pair Lone pair/ bonding pair

Answer 26

Lone pair/ lone pair = biggest Lone pair/ bonding pair = second biggest Bonding pair/ bonding pair = smallest

Question 27

Describe electron repulsion theory (including bond angles)

Answer 27

No lone pairs = 109.5° 1 lone pair = 107.0° 2 lone pairs = 104.5°

Question 28

what is the shape of a molecule that has 2 electron pairs around a central atom? (And bond angle)

Answer 28

A linear molecule eg. CO2 180°

Question 29

What is the shape of a molecule that has 3 electron pairs around a central atom with no lone pairs? (And bond angle)

Answer 29

Trigonal planar 120°

Question 30

What is the name of a molecule that has 4 electron pairs around a central atom? (No lone pairs) (and bond angle)

Answer 30

Tetrahedral 109.5°

Question 31

What is the name of a molecule that has 4 electron pairs and 1 lone pair? (And bond angle?)

Answer 31

Trigonal pyramidal 107° (not by lone pair)

Question 32

What is the name of a molecule that has 4 electron pairs and 2 lone pairs? (And bond angle?)

Answer 32

Non linear (Bent) 104.5° only between two angles (not between lone pairs idk either)

Question 33

What is the name of a molecule that has 5 electron pairs around a central atom with no lone pairs? (And bond angles)

Answer 33

Trigonal bipyramidal 120° & 90° idk ether babe

Question 34

What is the name for a molecule which has 6 electron pairs around a central atom and no lone pairs? And bond angle

Answer 34

Octahedral 90°

Question 35

Define electronegativity

Answer 35

An atoms ability to attract the electron pair in a covalent bond

Question 36

What is the most electronegative atom?

Answer 36

Flourine

Question 37

How is electronegativity measured?

Answer 37

On the Pauling scale- greater the Pauling value the greater the electronegativity

Question 38

How does electronegativity (groups and periods)

Answer 38

Increases across periods and decreases down groups (ignoring Nobel gases)

Question 39

What happens to the electrons in a covalent bond between two atoms of different electronegativity’s?

Answer 39

Pulled towards the more electronegative atom Makes the bond polar

Question 40

In a polar bond, what does the difference in electronegativity cause?

Answer 40

A permanent dipole

Question 41

What is a dipole?

Answer 41

a difference in charge between two atoms caused by a shift in electron density in the bond

Question 42

What does a greater difference in electronegativity cause?

Answer 42

The more polar the bond

Question 43

What are the bonds in diatomic gases (Cl2, H2) (polar or non polar)

Answer 43

Non polar- equal electronegativity

Question 44

What happens to the dipoles on a molecule if it is symmetrical?

Answer 44

Cancel each other out eg. CO2 Becomes non polar

Question 45

What happens to the dipoles if a molecule is unsymmetrical?

Answer 45

Do not cancel Will have a dipole Eg. H2O

Question 46

Explain why only bonds between single elements (eg. Diatomic gases) can be purely covalent?

Answer 46

Electronegativity difference is zero so bonding electrons can be arranged completely evenly within the bond

Question 47

Roughly how many compounds are completely ionic?

Answer 47

Very few

Question 48

How can you use electronegativity to predict which type of bonding?

Answer 48

Higher the difference in electronegativity the more ionic in character the bonding will be

Question 49

What are most compounds bonding?

Answer 49

Somewhere between ionic and covalent Often have ionic and covalent properties

Question 50

What are the three types of intermolecular forces?

Answer 50

Induced dipole- dipole interactions (London) Permanent dipole- dipole interactions Hydrogen bonding- strongest type

Question 51

Where are induced dipole-dipole forces found?

Answer 51

Between all atoms and molecules (even Nobel gases)

Question 52

What causes induced dipole-dipole forces?

Answer 52

Electrons in charge clouds are always moving- at any particular second the electrons are likely to be more to one side than the other- at this moment the atom will have a TEMPORARY DIPOLE This can cause a ‘domino effect’- (cause another temporary dipole to form on a neighbouring atom)

Question 53

How do dipole-dipole forces vary in strength?

Answer 53

Larger molecules have larger electron clouds therefore stronger induced dipole-dipole forces

Question 54

Do liquids with stronger induced dipole-dipole have higher boiling points?

Answer 54

Yes- more energy to overcome intermolecular forces, so particles can escape from the liquid surface

Question 55

Can induced dipole-dipole forces hold molecules together in a lattice?

Answer 55

Yes Iodine held together in pairs by strong covalent bonds to form I2 molecules Molecules then held in a weak lattice by induced dipole-dipole attractions

Question 56

What interactions do polar molecules form and how?

Answer 56

Permanent dipole-dipole interactions Sigma charges on polar molecules causes weak electrostatic forces between molecules

Question 57

Which is the strongest intermolecular force?

Answer 57

Hydrogen bonding

Question 58

When can hydrogen bonding only happen?

Answer 58

When hydrogen is covalently bonded to one of fluorine, nitrogen, oxygen

Question 59

what property does hydrogen have? In link to polarity LOL

Answer 59

High charge density

Question 60

How is the bond between hydrogen and one of Fl, O, N, POLARISED?

Answer 60

High charge density on hydrogen as its small and H, O, Fl are very electronegative So it’s polarised that a weak bond forms between the hydrogen of one molecule and a lone pair of electrons on the FL, H, O, or another molecule

Question 61

Give to examples of molecules that use hydrogen bonding

Answer 61

Water and ammonia

Question 62

What effect does hydrogen bonding have on BP and FP?

Answer 62

Higher BP Higher freezing point

Question 63

What effect does hydrogen bonding have on solubility?

Answer 63

Soluble in water

Question 64

How is ice less dense than water?

Answer 64

In ice H2O is held together in a lattice by hydrogen bonds. When it melts hydrogen bonds are broken, so ice has more hydrogen bonds than liquid water Since H2 bonds are long this makes ice less dense than liquid H2O

Question 65

What usually determines the boiling point of a substance?

Answer 65

Induced dipole-dipole forces (unless the molecule forms H2 bonds)

Question 66

Why are polar molecules soluble in water?

Answer 66

Water is polar, so only tends to dissolve other polar substances Eg. Ammonia can form hydrogen bonds so soluble

Question 67

Why don’t simple covalent compounds conduct electricity?

Answer 67

Overall the molecules are uncharged

Question 68

Why do simple covalent compounds have low melting and boiling points?

Answer 68

They have weak intermolecular forces- not much energy needed to break Usually liquids or gases at room temp

Question 69

Do covalent bonds break during melting and boiling?

Answer 69

No Break/ overcome intermolecular forces NOT the covalent bonds EXCEPT GIANT MOLECULAR SUBSTANCES