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CHEMISTRY Module 2: Foundation In Chemistry > 2.2 Electrons, Bonding And Structure > Flashcards

2.2 Electrons, Bonding And Structure Flashcards

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1
Q

Configuration of electrons for the first four shells

A

2, 8, 18, 32

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2
Q

What is an atomic orbital?

A

A region around the nucleus that can hold up to 2 electrons, with opposite spins.

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3
Q

What shape is an s orbital

A

Sphere

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4
Q

Which shells contain s orbitals

A

All 4 shells contain one s orbital

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5
Q

What shape is a p-orbital

A

Dumb-bell

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6
Q

What are the three p-orbitals

A

Px
Py
Pz

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7
Q

Which shells contain p-orbitals

A

2nd, 3rd and 4th subshells contain 3 p-orbitals

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8
Q

Which shells contain d-orbitals

A

3rd and 4th subshells contain 5 d-orbitals

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9
Q

How do sub-shells fill according to energy levels

A

In each shell, new type of sub-shell has higher energy
Highest energy level in 3rd shell overlaps with lowest energy level in 4th shell

So
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 4d

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10
Q

Why do electron pairs in a cloud have opposite spins

A

They’re negatively charged and repel each other
Opposite spins helps to counteract repulsion

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11
Q

Why do orbitals with the same energy occupy singly first

A

Prevents repulsion between paired electrons

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12
Q

Ionic bonding definition

A

Electrostatic attraction between positive and negative ions

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13
Q

How are giant ionic lattices formed

A

Oppositely charged ions attract each other in all directions equally

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14
Q

Example of a giant ionic lattice

A

NaCl

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15
Q

Ionic compounds melting and boiling points

A

High temperatures needed to provide energy needed to overcome strong electrostatic attraction between ions.
Therefore , high melting and boiling points

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16
Q

Solubility in ionic compounds

A

Many dissolve in polar solvents (water), water molecules break down the lattice and surround each ion in solution
However, with compounds made of ions with large charges, ionic attraction may be too strong for water to be able to break down the lattice structure, then would not be soluble.

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17
Q

Electrical conductivity in ionic compounds

A

Don’t conduct electricity in a solid state as ions are in a fixed position in giant ionic lattice and no mobile charge carriers.
Once molten/ aqueous ionic compounds conduct electricity as solid ionic lattice breaks down and ions are free to move as mobile charge carriers

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18
Q

Definition of covalent bonding

A

Strong electrostatic attraction between shared pair of electrons and the nuclei of the bonded atoms.

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19
Q

How many covalent bonds does carbon form

A

4

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20
Q

How many covalent bonds does nitrogen form

A

3

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21
Q

How many covalent bonds does oxygen form

A

2

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22
Q

How many does covalent bonds does hydrogen form

A

1

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23
Q

Configuration of BF3

A

3 covalent bonds, only 6 electrons on outer shell of boron

24
Q

What is a dative covalent/ coordinate bond

A

Shared pair of electrons has been supplied by one of the bonding atoms only

25
Q

Example of dative covalent bonding

A

NH4+

26
Q

What is average bond enthalpy

A

Measurement of covalent bond strength

27
Q

Shape name for 4 bonded pairs

A

Tetrahedral

28
Q

Bond angles for tetrahedral shape

A

109.5

29
Q

Shape for 3 bonded pairs and 1 lone pair

A

Pyramidal

30
Q

Pyramidal shape bond angles

A

107

31
Q

Shape for 2 bonded pairs and 2 lone pairs

A

Non-linear

32
Q

Angles in non-linear shape

A

104.5

33
Q

Shape for 2 bonded pairs

A

Linear

34
Q

Angles in linear shape

A

180

35
Q

Shape for 3 bonded pairs

A

Trigonal planar

36
Q

Angles in trigonal planar shape

A

120

37
Q

Shape for 6 bonded pairs

A

Otahedral

38
Q

Angles in octahedral shape

A

90

39
Q

How are the different repulsions by different electron pairs ordered

A

2 bonded < one bonded one lone < 2 lone

40
Q

Why does the presence of lone pairs decrease the angle

A

Lone pairs repel more strongly than bonded, so lone pairs repel bonded pairs slightly closer together which decreases the bond angle

41
Q

Definition of electronegativity

A

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

42
Q

Covalent polar bonds in terms of electronegativity

A

The bonded electron pair is shared unequally between bonded atoms due to different electronegativity values.
Creates a permanent dipole.

43
Q

Polar molecules in terms of electronegativity

A

For molecules with more than one polar bonds there will be multiple dipoles and depending on the shape they either will or wont cancel eachother out.
If the dipoles don’t cancel out, it is a polar molecule.

44
Q

What are London forces

A

Weak intermolecular forces that exist between all molecules

45
Q

How are London forces formed

A

Movement of electrons produces changing dipoles in a molecule and an instantaneous dipole exists which induces a dipole on a neighbouring molecule this induction continues

46
Q

How does the strength of London forces change

A

In a molecule with more electrons, there’s larger instantaneous and induced dipoles, greater induced interactions and stronger attractive forces

47
Q

What are permanent dipole-dipole interactions

A

Forces that act between the permanent dipoles in different polar molecules
Stronger than London forces

48
Q

What happens in a simple molecular lattice

A

Molecules held in place by weak intermolecular forces
Atoms within each molecule bonded strongly by covalent bonds

49
Q

Melting and boiling points of simple molecular substances

A

In a lattice, weak IMF broken easily, low melting and boiling points

50
Q

Solubility of non-polar molecular substances

A

IMF form between non-polar solvent, these interactions weaken and break IMF in simple molecular lattice, compound dissolves.
Little interactions with polar solvents, IMF within polar solvent too strong to break, compound doesn’t dissolve

51
Q

Solubility of polar simple molecular substances

A

Polar solute and solvent molecules can attract each other, solubility depends on strength of dipole

52
Q

Electrical conductivity in simple molecular structures

A

No mobile charged particles, nothing to complete electrical circuit, non-conductors

53
Q

Where can hydrogen bonds form

A

Between molecules containing an electronegative atom with a lone pair (oxygen nitrogen fluorine)
And an hydrogen atom attached to the electronegative atom (H-O H-N H-F)

54
Q

Why is ice less dense than water

A

Hydrogen bonds hold water molecules in open lattice structure, water molecules further apart in ice than water

55
Q

Melting and boiling points of water

A

Relatively high due to hydrogen bonds
More energy is needed to break the H bonds, as it has those as well as London forces

CHEMISTRY Module 2: Foundation In Chemistry (5 decks)

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