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2016 GAMSAT > Chemistry - Atoms, Bonds and Groups - F321 - Electrons, Bonding and Structure (2) > Flashcards

Chemistry - Atoms, Bonds and Groups - F321 - Electrons, Bonding and Structure (2) Flashcards

1
Q

Define the first ionisation energy of an element.

A

The first ionisation energy of an element is the energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions.

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2
Q

What are plasma televisions made from?

A

Plasma televisions are made of a mixture of positive and negative ions.

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3
Q

What provides evidence that electrons are arranged in shells?

A

Ionisation energies provide evidenve that electrons are arranged in shells.

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4
Q

Which electrons are removed first?

A

Electrons in the outer shell are removed first as they experience the least attraction to the nucleus.

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5
Q

The nuclear attraction experienced by an electron depends on…:

A

The nuclear attraction experienced by an electron depends on:

  • atomic radius
  • nuclear charge
  • electron shielding
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6
Q

Define electron shielding

A

Electron shielding is the repulsion between electrons in different inner shells. Shielding reduces the net attractive force from the positive nucleus to the outer-shell electrons.

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7
Q

How many ionisation energies does each element have?

A

Each element has as many ionisation energies as it does electrons.

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8
Q

TRUE or FALSE

Each successive ionisation energy is smaller than the one before.

A

FALSE!

Each successive ionisation energy is larger than the one before.

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9
Q

What does a large difference in ionisation energies show?

A

A large difference n ionisation energies shows the electron has been removed from the next shell.

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10
Q

Define a shell.

A

A shell is a group of atomic orbitals with the same principle quantum number, n. Also known as a main energy level.

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11
Q

Define principle quantum number.

A

Principle quantum number, n, is a number representing the relative overall energy of each orbital, which increases with distance from the nucleus. The group of orbitals with the same n-value are referred to as electron shells or energy levels.

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12
Q

How many electrons can be held in the first shell?

A

2 electrons can be held in the first shell.

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13
Q

How many electrons can be held in the second shell?

A

8 electrons can be held in the second shell.

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14
Q

How many electrons can be held in the third shell?

A

18 electrons can be held in the third shell.

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15
Q

How many electrons can be held in the fourth shell?

A

32 electrons can be held in the fourth shell.

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16
Q

What is the formula for the number of electrons in each shell?

A

2n^2 electrons

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17
Q

Define an atomic orbital.

A

An atomic orbital is a region within an atom that can hold up to two electron with opposite spins.

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18
Q

What shape is an s-orbital?

A

An s-orbital has a spherical shape.

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19
Q

How many electrons can each orbital hold?

A

Each orbital can hold 2 electrons.

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20
Q

Define a sub-shell.

A

A sub-shell is a group of the same type of atomic orbitals (s, p, d, f) within a shell.

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21
Q

Electron configuration can be worked out using what principle?

A

Electron configuration can be worked out using the Aufbau principle.

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22
Q

What are the key points of working out electron configuration according to the rules of the Aufbau principle?

A
  • electrons are added one at a time to ‘build up’ the atoms
  • the lowest available energy level is filled first
  • each energy level must be full before the next higher energy level starts to fill
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23
Q

The ……. the principle quantum number, n, the further the shell from the nucleus.

A

The higher the principle quantum number, n, the further the shell from the nucleus.

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24
Q

What are the only six elements that exist as unbonded atoms?

A 
Helium
Neon
Argon
Krypton
Xenon
Radon

The noble gases.

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25
Q

Noble gases make up what percentage of the air?

A

Noble gases make up ~1% of the air.

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26
Q

What is the most abundant noble gas in the air?

A

Argon is the most abundant noble gas in the air.

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27
Q

What is the use of helium?

A

Helium is used in airships.

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28
Q

What is the use of neon?

A

Neon is used in advertising signs.

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29
Q

What is the use of argon?

A

Argon is used in filament lightbulbs.

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30
Q

What is the use of krypton?

A

Krypton is used in lasers for eye surgery.

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31
Q

What is the use of xenon?

A

Xenon is used in car headlights.

32
Q

Define an ionic bond.

A

An ionic bond is the electrostatic attraction between oppositely charged ions.

33
Q

Define a giant ionic lattice.

A

A giant ionic lattice is a three-dimensional structure of oppositely charged ions, held together by strong ionic bonds.

34
Q

How do all ionic compounds exist in their solid state?

A

All ionic compounds exist as a giant ionic lattice in the solid state.

35
Q

Elements in the same …. of the periodic table have the same number of outer shell electrons and react in similar ways.

A

Elements in the same group of the periodic table have the same number of outer shell electrons and react in similar ways.

36
Q

Define a group in the periodic table.

A

A group is a vertical column in the periodic table. Elements in the same group have similar chemical properties and their atoms have the same number of outer shell electrons.

37
Q

Which atoms do not usually form ions?

A

Beryllium, boron, carbon and silicon do not normally form ions as too much energy is needed to transfer the outer shell electrons to form ions.

38
Q

Define a covalent bond.

A

A covalent bond is a bond formed by a shared pair of electrons.

39
Q

Define a lone pair.

A

A lone pair is an outer shell pair of electrons that is not involved in chemical bonding.

40
Q

Define a dative covalent bond.

A

A dative covalent bond or coordinate bond is a shared pair of electrons which has been provided by one of the bonding atoms only.

41
Q

What is anothe rname for a dative covalent bond?

A

A dative covalent bond is also known as a coordinate bond.

42
Q

How can a dative covalent bond be written?

A

A –> B

Where the arrow represents which atoms has donated a lone pair of electrons to form the dative covalent bond.

43
Q

When an acid is added to water, what ions does the water form?

A

When an acid is added to water, the water forms oxonium ions H3O+

44
Q

What shape will a molecule with three electron pairs around the central atom form?

A

A molecule with three electron pairs around the central atom will have a trigonal planar shape.

45
Q

What shape will a molecule with four electron pairs around the central atom form?

A

A molecule with four electron pairs around the central atom will have a tetrahedral shape.

46
Q

What shape will a molecule with six electron pairs around the central atom form?

A

A molecule with six electron pairs around the central atom will have an octahedral shape.

47
Q

What is the bond angle in a molecule of trigonal planar shape?

A

The bond angle in a molecule of trigonal planar shape is 120o

48
Q

What is the bond angle in a molecule of tetrahedral shape?

A

The bond angle in a molecule of tetrahedral shape is 109.5o

49
Q

What is the bond angle in a molecule of octahedral shape?

A

The bond angle in a molecule of octahedral shape is 90o

50
Q

How much does each lone pair reduce the bond angle by?

A

Each lone pair reduces the bond angle by ~2.5o

51
Q

Define electronegativity.

A

Electronegativity is a measure of the attraction of a bonded atom for the pair of electrons in a covalent bond.

52
Q

A charge difference between two bonded atoms such as H-Cl is called what?

A

A charge difference between two bonded atoms such as H-Cl is called a permanent dipole.

53
Q

Define a permanent dipole.

A

A permanent dipole is a small charge difference across a bond that results from a difference in the electronegativities of the bonded atoms.

54
Q

What scale is used to measure electronegativity?

A

The Pauling scale is used to measure electronegativity.

55
Q

At room temperature, all ionic compounds are what?

A

At room temperature, all ionic compounds are solid.

56
Q

Define an intermolecular force

A

An intermolecular force is an attractive force between neighbouring molecules.

57
Q

What are the three types of intermolecular force?

A

The three types of intermolecular force are:

  • Hydrogen bonds
  • Permanent dipole -dipole
  • van der Waals’
58
Q

Define van der Waals’ forces.

A

van der Waals’ forces are attractive forces between induced dipoles in neighbouring molecules.

59
Q

What causes can der Waals’ forces?

A

van der Waals’ forces are caused by the movement of electrons in shells.

60
Q

What increases the number/strength of van der Waals’ forces?

A

van der Waals’ forces increase with the number of electrons.

61
Q

What are the only attractive intermolecular forces that act between non-polar molecules?

A

van der Waals’ forces are the only attractive intermolecular forces acting between non-polar molecules.

62
Q

What percentage of the strength of a covalent bond is an hydrogen bond?

A

An hydrogen bond is about 5% of the strength of a covalent bond.

63
Q

Why do hydrogen bonds make ice less dense than water?

A

Hydrogen bonds make ice less dense than water because hydrogen bonds hold the water molecules apart so ice has an open lattice structure that collapses as it melts.

64
Q

Define metallic bonding.

A

Metallic bonding is the electrostatic attraction between positive metal ions and delocalised electrons.

65
Q

Delocalised electrons are shared between how many atoms?

A

Delocalised electrons are shared by more than two atoms.

66
Q

Define a giant metallic lattice.

A

A giant metallic lattice is a three-dimensional structure of positive ions and delocalised electrons, bonded together by strong metallic bonds.

67
Q

When are ionic compounds conductors of electricity?

A

When melted or dissolved in water ionic compounds are conductors of electricity.

68
Q

Ionic lattices dissolve in what?

A

Ionic lattices dissolve in polar solvents.

69
Q

Define a simple molecular lattice.

A

A simple molecular lattice is a three-dimensional structure of molecules, bonded together by weak intermolecular forces.

70
Q

Are simple molecular lattices conductors of electricity?

A

Simple molecular lattices are non-conductors of electricity.

71
Q

Do simple molecular lattices have relatively high or low boiling and melting points?

A

Simple molecular lattices have relatively low melting and boiling points.

72
Q

What are simple molecular lattices soluble in?

A

Simple molecular lattices are soluble in non-polar solvents (eg hexane).

73
Q

Define a giant covalent structure.

A

A giant covalent structure is a three-dimensional structure of atoms, bonded together by strong covalent bonds.

74
Q

What molecules have giant covalent structures?

A

Graphite and diamond have giant covalent structures.

75
Q

What shape is diamond?

A

Diamond has a tetrahedral structure.

76
Q

What shape is graphite?

A

Graphite has a hexagonal layer structure.

2016 GAMSAT (19 decks)

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