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Chemistry > Electrons, Bonding and Structure > Flashcards

Electrons, Bonding and Structure Flashcards

(59 cards)

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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?

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A

linear shape, 180° bond angle

25
What is the shape and bond angle of a molecule with 3 bond pairs and no lone pairs?
triganol planar shape, 120° bond angle
26
What is the shape and bond angle of a molecule with 4 bond pairs and no lone pairs?
tetrahedral shape, 109.5° bond angle
27
What is the shape and bond angle of a molecule with 5 bond pairs and no lone pairs?
trigonal bipyramidal shape, 90° and 120° bond angle
28
What is the shape and bond angle of a molecule with 6 bond pairs and no lone pairs?
octahedral shape, 90° bond angle
29
What is the shape and bond angle of a molecule with 3 bond pairs and 1 lone pair?
pyramidal shape, 107° bond angle
30
What is the shape and bond angle of a molecule with 2 bond pairs and 2 lone pairs?
non-linear, 104.5° bond angle
31
Why does having more bond pairs and lone pairs change the shape of a molecule?
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
Why do lone pairs repel more than bond pairs?
Lone pairs are closer to the atom they are coming from, therefore having a much higher repulsion of nearby bond pairs.
33
What would a covalent bond that has each atom sharing more than 1 electron each be called?
a bond region
34
What is a dative covalent bond?
a bond between 2 atoms where only 1 atom donates a lone pair of electrons to form the bond
35
What is electronegativity?
The measure of a tendancy for an atom of an element to attract the bond pair of electrons towards itself
36
What is the scale of electronegativty called?
The Pauling Scale
37
What is the most and least electronegative regions of the periodic table?
Most: Elements near Floruine, except the Noble gasses Least: Elements near the bottom left of the periodic table
38
What happens if two atoms of a very similiar electronegativity bond together?
Nothing, a normal covalent bond forms and the bond pair stays in the middle of the 2 atoms
39
What happens if two atoms of a medium difference of electronegativity bond together?
The bond pair is "pulled" towards the more electronegative atom, forming a polar bond
40
What happens if two atoms of a very large difference of electronegativity bond together?
The bond pair is fully "pulled" towards the more electronegative atom forming an ionic bond
41
What are the ranges for different types of bonds compared to differences of electronegativity?
<0.4 is a non-polar bond >0.4 is a polar bond >2.0 is an ionic bond
42
What is a polar bond?
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
What is a dipole?
An overall difference of charge in a molecule with a direction of the difference of charge towards the negative charge.
44
How is a permanent dipole formed?
When there are polar bonds in a molecule that don't cancel because the molecule or bonds across the molecule aren't symetrical
45
What is a polar molecule?
A molecule with an overall permanent dipole
46
What is an instantaneous dipole?
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
What is an induced dipole?
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
How are simple molecules held together?
Intermolecular forces that are caused by either permanent dipole-dipole interactions or induced dipole-dipole interactions
49
Which simple molecules have a higher boiling point: molecules with permanent dipole-dipole interactions or molecules with induced dipole-dipole interactions and why?
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
Why does H2O have such a high boiling point compared to other group 6 hydrides?
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
What are some properties of molecules with hydrogen bonds and why?
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
Do induced dipole-dipole interactions exist with molecules held together with permanent dipole-dipole interactions or hydrogen bonds?
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
What is another name for induced dipole-dipole interactions?
London Forces
54
What is another name for intermolecular forces?
van der Waal's forces
55
Why do some substances dissolve in water and others don't?
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
Can non-polar substances dissolve in anything?
yes, in non-polar liquids
57
What substances can dissolve in what liquids?
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
What are the energy per mole of each type of intermolecular force?
Hydrogen bond: 10-40 kJ/mol Permanent dipoles: 3-25 kJ/mol London Forces: 1-10 kJ/mol
59
Are intermolecular forces stronger or weaker than bonds?
much, much, much weaker than covalent bonds and ionic bonds

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