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Chemistry Module 2 > Electrons, Bonding and Structure > Flashcards

Electrons, Bonding and Structure Flashcards

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1
Q

describe an ionic bond

A

electrons are transferred from the metal atom to the non-metal atom, oppositely charged ions are formed and held together by electrostatic attraction
metal ion = +, non-metal ion= -

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2
Q

describe a giant ionic lattice

A

each ion is surrounded by oppositely charged ions
these ions attract each other from all directions
when in a liquid state the ions are free to move so can conduct electricity

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3
Q

describe sodium chloride

A

giant ionic compound, each Na + ion surrounded by 6 Cl- ions and each cl- ion is surrounded by 6 Na+ ions

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4
Q

what does the size of an ionic compound depend on?

A

the size depends on the amount of ions invovled

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5
Q

Why do ionic bonds have high melting/boiling points?

A

ionic compounds are solid at room temperature and a large amount of energy is needed to break strong electrostatic bonds that hold oppositely charged ions together therefore increasing the melting points
- the greater the charge the stronger to electrostatic forces between the ions and the more energy is required to break them

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6
Q

How does electrical conductivity work?

A

in a solid lattice the ions are in fixed positions and cannot move therefore there is no conduction
in melted or dissolved, the broken down lattice and ions are free to move and therefore can conduct electricity

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7
Q

What makes up covalent bonds?

A

non-metals and non-metals

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8
Q

How does covalent bonding work?

A

the electron pair occupies the space between the two atomic nuclei, the negatively charged shared pair of electrons is attracted to the positive charges of both nuclei, this attraction overcomes the repulsion between 2 positively charged nuclei and therefore holding the non-metals together

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9
Q

What is a single covalent bond?

A

a single bond is when atoms are bonded by one shared pair of electrons

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10
Q

What is a lone pair of electrons?

A

this is an outer shell pair of electrons that are not involved in chemical bonding

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11
Q

What is multiple covalent bonding?

A

some non-metallic atoms can share more than one pair of electrons to form a multiple bond

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12
Q

what is average bond enthalpy?

A

the amount of energy required to break a bond

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13
Q

Why is bond breaking always positive?

A

bond breaking is endothermic change which requires energy

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14
Q

The bigger the average bond enthalpy value…

A

the more energy required to break the bond

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15
Q

What sort of molecules form simple structures?

A

there made up of small simple non-mental molecules

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16
Q

What sort of bonding is present in simple structures?

A

covalent bonding, they have strong covalent bonds but weak intermolecular forces

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17
Q

What is the definition of a simple structure lattice?

A

a 3-dimensial structure of molecules held together by weak intermolecular forces

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18
Q

why do simple structures have low melting and boiling points?

A

the intermolecular forces are weak between molecules and a small amount of energy can break them, the covalent bonds are not broken

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19
Q

Do simple structures conduct electricity?

A

No, there are no free charged particles

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20
Q

what do simple structures dissolve in and why?

A

non-polar solvents, between covalent molecules and non-polar structures weak London forces form which break down the lattice and dissolves the solvent

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21
Q

How our giant covalent structures defined?

A

a 3-deimensial structure of atoms that are all bonded together by strong covalent bonds

22
Q

Why do giant structures have high melting points?

A

need to break strong covalent bonds, this requires a lot of energy

23
Q

Do giant structures conduct electricity?

A

no, this is because they have no free charged particles

24
Q

describe graphite

A

has layers of carbon atoms which have weak intermolecular forces between them that can easily be broken this is why the layers can slide over one another and why graphite is soft
can conduct electricity as it has free delocalised electrons which travel parallel to the layers when a charge is applied

25
Q

Why don’t giant structures dissolve?

A

the structures do not dissolve as the bonds between the ions are too strong to break

26
Q

what is dative bonding?

A

a shared pair of electrons which have been provided by only one of the bonding atoms, it is also known as a co-ordinate bond

27
Q

What is the expansion of the octet?

A

when more than 4 electrons may pair up in bonding

28
Q

How many bonds can group 15 form?

A

3 or 5

29
Q

How many bonds can group 16 form?

A

2, 4, 6

30
Q

How many bonds can group 17 form?

A

1, 3, 5

31
Q

modifying the octet rule?

A

unpaired electrons pair up

the maximum number of electrons that can pari up is equivalent to its outer shell

32
Q

What is the electron pair repulsion theory?

A

the shape of a molecular ion is determined by the number of electron pair in the outer shell surrounding the central atom

33
Q

How is the electron shape decided?

A

as the electrons all have negative charge each pair repels the other electron pair therefore the shape allows all the pair of electrons to be far apart as possible

34
Q

if the bonding pair has one or two pairs of electrons what is its name and what is its angle

A

linear, 180

35
Q

if the boding pair is 3 pairs of electrons what is its name and what is its angle?

A

trigonal planar, 120

36
Q

if the boding pair is 4 pairs of electrons what is its name and what is its angle?

A

tetrahedral, 109.5

37
Q

if the boding pair is 5 pairs of electrons what is its name and what is its angle?

A

trigonal bipyramid, 120, 90

38
Q

if the boding pair is 6 pairs of electrons what is its name and what is its angle?

A

octahedral, 90

39
Q

what is the bond angle and name of a molecule which has 3 bonding pairs and one lone pair

A

pyramidal, 107

40
Q

what is the name and bond angle of a molecule which has 2 bonding pairs and 2 lone pairs

A

non-linear, 104.5

41
Q

what is the effect of a lone pair on molecule shapes?

A

the lone pairs repel more than a bonded pair as they are more electron dense, therefore they reduce the bond angle by about 2.5 degrees due to the extra repulsive effect

42
Q

when do non-polar bonds happen?

A

when electrons are evenly shared

43
Q

when do polar bonds happen?

A

when electrons are not evenly shared and one of the atoms will attract the electrons more
- this makes a slight charge difference called a permanent diploe

44
Q

what is a permanent diploe

A

a small charge difference across a bond that results from the difference in electronegative of the bonded atoms

45
Q

Whats the difference between covalent bonding and dative covalent bonding?

A

In a covalent bond the two elements bonding are providing one electron to the shared pairs whereas in a dative covalent bond one of the elements provides both electrons for the shared pair

46
Q

Why might a molcules contain polar bonds but the molecules are non-polar?

A

Each bond is polar where one element is + and one element being -
Overall structure is symmetrical so the x dipoles cancel out

47
Q

In which quantum shells do s-orbitals appear?

A

Every quantum shell

48
Q

In which quantum shells do p-orbitals appear?

A

All quantum shells apart from the 1st

49
Q

Which three rules apply when filling energy levels?

A

Electrons enter the lowest energy level available
Two electrons in the same orbital must have opposite spin
Electrons will try and remain unpaired to reduce electrostatic repulsion and increase stability

50
Q

Do ionic bonds dissolve?

A

Most ionic compounds dissolve in water as water molecules are polar and attracted to the charged ions
An ionic substance only dissolves if more energy is released by separating the bonds then breaking the bonds

51
Q

What are the three factors that effect electronegativity?

A

Atomic radius
Shielding
Nuclear charge

52
Q

What is the link between electronegativity and bonding?

A

Compounds made up of elements with a large difference in electronegativity will be ionic, if they are similar in electronegativity they are likely to be covalent

Chemistry Module 2 (9 decks)

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