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CHE144 > Matter > Flashcards

Matter Flashcards

1
Q

When can the ground state be found?

A

When all the electron orbitals are filled.

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2
Q

What are ions?

A

Atoms with a charge imbalance.

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3
Q

What is a valence shell?

A

The outermost shell of electrons for an atom.

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4
Q

What is electron affinity?

A

The charge required to add an electron.

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5
Q

What is ionisation energy?

A

The energy required to remove an electron.

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6
Q

Which atoms have the greatest 1st ionisation energy?

A

Those at the top right of the periodic table.

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7
Q

What happens to the size of the atomic radii when an electron is lost?

A

Atomic radii decreases because of the + charge.

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8
Q

What is the only force between particles?

A

Electrostatic forces

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9
Q

What are three examples of electrostatic forces?

A

Covalent bonds, ionic bonds and metallic bonds

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10
Q

What two bonds share electrons?

A

Covalent and ionic.

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11
Q

What happens to electrons in ionic bonding?

A

The tend to reside around the stronger of the two atoms.

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12
Q

What happens to electrons in covalent bonding?

A

They’re shared between two atoms.

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13
Q

When is a bond considered ionic?

A

When the electronegativity is greater than 2.0

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14
Q

What is the speed of light?

A

3.00x10^8m/s

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15
Q

What is the relationship between absorption and emission spectra?

A

They’re opposites.

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16
Q

What is a chromophore?

A

The part of the atom that interacts with electromagnetic radiation.

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17
Q

What is happening when something appears blue?

A

The object is absorbing all light but blue.

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18
Q

What is a general characteristic of chromophores in the visible spectrum?

A

They generally have a lot of double bonds.

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19
Q

What is a congugated system?

A

A carbon system with alternating single and double bonds.

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20
Q

Define spectroscopy?

A

A general term used for the methods of determining molecular structure.

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21
Q

When can two electrons occupy the same space?

A

When they are out of phase with each other.

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22
Q

Is matter infinitely divisible?

A

No

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23
Q

What is the uncertainty principal?

A

The smaller something is, the less you can know about it.

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24
Q

How many electrons can p-sub shells hold?

A

6

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25
How many electrons can d-subshells hold?
10
26
How many electrons can s-subshells hold?
2
27
What is hybridisation?
The process of mixing two atomic orbitals to get a molecular orbital.
28
What is a Z isomer?
The two high priority groups are on the same side of the double bond. (cis)
29
What is an E isomer?
The two high priority groups are on the opposite side of the double bond (trans).
30
What are enantioners?
Molecules that are mirror images that form around a chiral carbon.
31
What is a chiral carbon?
A carbon atom with four different groups attached.
32
What is an R isomer?
A molecule that spins clockwise when the lowest priority functional group faces away from you.
33
What is an S isomer?
A molecule that spins anticlockwise when the lowest priority functional group faces away from you.
34
What is micibility?
The solubility of a liquid in another liquid.
35
When is a solution formed?
When a substance disperses uniformly throughout another.
36
What are three intermolecular forces?
Dispersion, dipole-dipole and hydrogen bonding.
37
What is solvation?
The interaction between solute and solvent.
38
What is hydration?
A solution where the solvent is water.
39
What is the limitation of the Bohr model?
The Bohr model can explain the line spectra for H but not for any other atom.
40
What did Bohr suggest about electrons? (2)
Electrons exist in discrete energy levels and energy is involved in moving an electron from one level to another.
41
What are the letters used for electron orbitals (in order, give examples)?
S P D F (1s,2s,2p,3s,3p,3d,4s,4p,4d,4f)
42
What is an electron shell?
A collection of orbitals with the same value for n.
43
How many electrons can each shell hold?
n^2
44
What shape are p-orbitals?
Dumbbell shaped
45
What shape are d-orbitals?
4-leaf clover shaped apart from dz2 which has two lobes with a doughnut in the middle.
46
What would happen if there was no restriction for the values of quantum numbers?
All electrons would revert to the ground state.
47
How many electrons can be in each orbital?
2
48
What is Hund’s rule?
For degenerate orbitals, the lowest energy is attained when the number of electrons with the same spin is maximised.
49
What happens to first ionisation energy in each group?
First ionisation energy decreases with atomic number.
50
What electrons are removed first?
Those that are in the least filled orbital with the largest quantum number
51
Where are electrons added first?
The lowest quantum orbital that is partially filled.
52
What is Coulomb’s law?
The force of attraction between the nucleus and an electron depends on the net nuclear charge and the distance the electron is from the nucleus.
53
What happens to attraction in a many electron atom?
Electrons are simultaneously attracted to the nucleus but repelled by other electrons.
54
What is atomic radius?
Half of the distance between two identical nuclei that are chemically bonded.
55
How is atomic radius effected in each group?
Atom radius increases from top to bottom. As we go down electrons have a higher chance of being further away from the nucleus.
56
What happens to atomic radius in each period?
Atomic radius decreases from left to right. Increasing charge draws valence electrons closer.
57
Define isoelectric series.
A group of icons containing the same number of electrons.
58
What group has the lowest first ionisation energy?
Alkali metals
59
What happens to first ionisation energy in each period?
First ionisation energy increases with atomic number.
60
What are the three types of chemical bond?
Ionic, covalent and metallic
61
What are ionic bonds?
Ionic bonds occur due to the differing bonds between adjacent ions.
62
What happens in covalent bonding?
Two particles share electrons.
63
What happens in metallic bonds?
In metallic bonds each atom is bonded to several neighbouring atoms and electrons are free to move around the structure.
64
Which electrons are involved in bonding?
Valence electrons
65
Which sub shells are full in an octet?
S and P
66
What is a formal charge?
A formal charge is the charge a molecule would have if all the atoms in it were equally electronegative.
67
What is a resonance Lewis structure?
Versions of the same molecule with different electron configurations.
68
What is electron domain geometry?
The arrangement of electrons around a central atom
69
What happens when all electron domains are bonds?
Molecular geometry = electron geometry
70
What happens to bond angles when lone pairs of electrons are present?
The bond angles get smaller
71
Which has a higher repulsion: non-bonding pairs or bonding pairs?
Non-bonding pairs
72
What is a sigma bond?
A covalent bond where electrons are dispersed evenly.
73
What is a pi-bond?
A bond with a sideways overlap of p-orbitals

CHE144 (4 decks)

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