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Chemistry > Electrons, Bonding and Structure > Flashcards

Electrons, Bonding and Structure Flashcards

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1
Q

What is a shell?

A

Where electrons are located around the atom

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2
Q

What is a sub-shell?

A

smaller structures that make up a shell

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3
Q

What is an orbital?

A

A shape of a sub-shell that can contain a single pair of electrons, both “doing 2 different things”

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4
Q

What are the orbitals in each shell?

A

First Shell: s orbital
Second Shell: s orbital, p orbitals
Third Shell: s orbital, p orbitals, d orbitals
Fourth Shell: s orbital, p orbitals, d orbitals, f orbitals

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5
Q

What is the Quantum Number?

A

The shell that a sub-shell is on

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6
Q

What is the elctron configuration?

A

simple detail of how many electrons are in each shell

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7
Q

What is the spdf configuration?

A

showing how many electrons are in each sub-shell of each shell.
quantum number | orbital shape | number of electrons e.g. 1s² is the first shell, the s orbital shape, with 2 electrons in the sub shell

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8
Q

What is an orbital shape?

A

Where an electron COULD probably be in the atom

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9
Q

What are the shapes of the s and p orbitals?

A

s - sphere around the nucleus
p - dumbell shape around the nucleus

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10
Q

How many electrons can be in each orbital?

A

2 electrons “doing different things”

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11
Q

What is an electron in boxes diagram?

A

Showing the paired electrons in each orbital in each sub-shell

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12
Q

How does a sub-shell fill?

A

Each electron is put seperatly into each orbital, then further electrons are put in pairs when all orbitals in the sub-shell have 1 electron

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13
Q

How can the spdf configuration be shortened?

A

By starting the configuration with the closest Noble Gas
e.g. Na = 1s² 2s² 2p⁶ 3s¹, this can be abreviated to [Ne] 3s¹

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14
Q

How many orbitals does each shell contain?

A

Shell 1: 1 s orbital
Shell 2: 1 s orbital, 3 p orbitals
Shell 3: 1 s orbital, 3 p orbitals, 5 d orbitals
Shell 4: 1 s orbital, 3 p orbitals, 5 d orbitals, 7 f orbitals

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15
Q

How many electrons can each shell hold?

A

Shell 1: 2
Shell 2: 8
Shell 3: 18
Shell 4: 32

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16
Q

What order do sub-shells fill?

A

1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f

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17
Q

What is an ionic bond?

A

A strong electrostatic attraction between oppositely charged ions

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18
Q

What is a giant ionic structure/lattice?

A

A structure/lattice that consists of atoms held together by ionic bonds that has no defined size and can repeat endlessly

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19
Q

What is a giant metallic structure?

A

A structure that consists of atoms held together by metallic bonds that has no defined size and can repeat endlessly

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20
Q

What is a giant covalent structure?

A

A structure that consists of atoms held together by covalent bonds that has no defined size and can repeat endlessly

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21
Q

What is a simple covalent molecule?

A

A molecule that consists of atoms held together by covalent bonds that has a small defined size

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22
Q

What is a covalent bond?

A

An electrostatic attraction between a negative shared pair of electrons and the positive nuclei of the bonded atoms

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23
Q

What is average bond enthalpy?

A

The required energy to break a mole of bonds in a molecule in the gaseous phase, averaged over the molecules containing that bond

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24
Q

What is the shape and bond angle of a molecule with 2 bond pairs and no lone pairs?

A

linear shape, 180° bond angle

25
Q

What is the shape and bond angle of a molecule with 3 bond pairs and no lone pairs?

A

triganol planar shape, 120° bond angle

26
Q

What is the shape and bond angle of a molecule with 4 bond pairs and no lone pairs?

A

tetrahedral shape, 109.5° bond angle

27
Q

What is the shape and bond angle of a molecule with 5 bond pairs and no lone pairs?

A

trigonal bipyramidal shape, 90° and 120° bond angle

28
Q

What is the shape and bond angle of a molecule with 6 bond pairs and no lone pairs?

A

octahedral shape, 90° bond angle

29
Q

What is the shape and bond angle of a molecule with 3 bond pairs and 1 lone pair?

A

pyramidal shape, 107° bond angle

30
Q

What is the shape and bond angle of a molecule with 2 bond pairs and 2 lone pairs?

A

non-linear, 104.5° bond angle

31
Q

Why does having more bond pairs and lone pairs change the shape of a molecule?

A

Each pair of electrons repel each other as far away as possible, this is known as the Valence Shell Electron Pair Repulsion theory (VSEPR theory)

32
Q

Why do lone pairs repel more than bond pairs?

A

Lone pairs are closer to the atom they are coming from, therefore having a much higher repulsion of nearby bond pairs.

33
Q

What would a covalent bond that has each atom sharing more than 1 electron each be called?

A

a bond region

34
Q

What is a dative covalent bond?

A

a bond between 2 atoms where only 1 atom donates a lone pair of electrons to form the bond

35
Q

What is electronegativity?

A

The measure of a tendancy for an atom of an element to attract the bond pair of electrons towards itself

36
Q

What is the scale of electronegativty called?

A

The Pauling Scale

37
Q

What is the most and least electronegative regions of the periodic table?

A

Most: Elements near Floruine, except the Noble gasses
Least: Elements near the bottom left of the periodic table

38
Q

What happens if two atoms of a very similiar electronegativity bond together?

A

Nothing, a normal covalent bond forms and the bond pair stays in the middle of the 2 atoms

39
Q

What happens if two atoms of a medium difference of electronegativity bond together?

A

The bond pair is “pulled” towards the more electronegative atom, forming a polar bond

40
Q

What happens if two atoms of a very large difference of electronegativity bond together?

A

The bond pair is fully “pulled” towards the more electronegative atom forming an ionic bond

41
Q

What are the ranges for different types of bonds compared to differences of electronegativity?

A

<0.4 is a non-polar bond
>0.4 is a polar bond
>2.0 is an ionic bond

42
Q

What is a polar bond?

A

When there is a difference in charge in a bond, with the negative “side” being towards the more electronegative atom and the positive “side” being towards the less electronegative atom

43
Q

What is a dipole?

A

An overall difference of charge in a molecule with a direction of the difference of charge towards the negative charge.

44
Q

How is a permanent dipole formed?

A

When there are polar bonds in a molecule that don’t cancel because the molecule or bonds across the molecule aren’t symetrical

45
Q

What is a polar molecule?

A

A molecule with an overall permanent dipole

46
Q

What is an instantaneous dipole?

A

A dipole formed from the random movement of electrons beign towards 1 side more than the other by pure chance causing a difference of charge forming a instantaneous dipole

47
Q

What is an induced dipole?

A

Dipoles that occur due to nearby dipoles existing, mainly seen with instantaneous dipoles causing nearby molecules to have induced dipoles for a split second

48
Q

How are simple molecules held together?

A

Intermolecular forces that are caused by either permanent dipole-dipole interactions or induced dipole-dipole interactions

49
Q

Which simple molecules have a higher boiling point: molecules with permanent dipole-dipole interactions or molecules with induced dipole-dipole interactions and why?

A

Molecules with permanent dipole-dipole interactions as they are constantly there and typically have a higher difference in charge than induced dipole-dipole interactions, which means they take more energy to overcome and have a higher boiling point

50
Q

Why does H2O have such a high boiling point compared to other group 6 hydrides?

A

The electronegativity difference between oxygen and hydrogen form a special permanent dipole, which has such a large charge difference it is referred to a hydrogen bond, this is also seen with HF and NH3

51
Q

What are some properties of molecules with hydrogen bonds and why?

A

Much higher boiling and melting point, due to hydrogen bonds needing much more energy to overcome
Expanding when freezing, due to hydrogen bonds wanting to be a large fixed distance away from each other

52
Q

Do induced dipole-dipole interactions exist with molecules held together with permanent dipole-dipole interactions or hydrogen bonds?

A

YES! Just because it has hydrogen bonding or permanent dipole-dipole interactions doesn’t mean it can’t have induced dipole-dipole interactions as well.

53
Q

What is another name for induced dipole-dipole interactions?

A

London Forces

54
Q

What is another name for intermolecular forces?

A

van der Waal’s forces

55
Q

Why do some substances dissolve in water and others don’t?

A

Water is a polar molecule, so other polar molecules will dissolve easily into water, while non-polar molecules wont dissolve really at all in water

56
Q

Can non-polar substances dissolve in anything?

A

yes, in non-polar liquids

57
Q

What substances can dissolve in what liquids?

A

Liquids that have polar molecules dissolve other substances with polar molecules
Liquids that have non-polar molecules dissolve other substances with non-polar molecules
Ionic substances dissolve into polar-liquids due to themselves having such a large charge difference between each ion

58
Q

What are the energy per mole of each type of intermolecular force?

A

Hydrogen bond: 10-40 kJ/mol
Permanent dipoles: 3-25 kJ/mol
London Forces: 1-10 kJ/mol

59
Q

Are intermolecular forces stronger or weaker than bonds?

A

much, much, much weaker than covalent bonds and ionic bonds

Chemistry (3 decks)

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