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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
Q

How many electrons can d-subshells hold?

A

10

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26
Q

How many electrons can s-subshells hold?

A

2

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27
Q

What is hybridisation?

A

The process of mixing two atomic orbitals to get a molecular orbital.

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28
Q

What is a Z isomer?

A

The two high priority groups are on the same side of the double bond. (cis)

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29
Q

What is an E isomer?

A

The two high priority groups are on the opposite side of the double bond (trans).

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30
Q

What are enantioners?

A

Molecules that are mirror images that form around a chiral carbon.

31
Q

What is a chiral carbon?

A

A carbon atom with four different groups attached.

32
Q

What is an R isomer?

A

A molecule that spins clockwise when the lowest priority functional group faces away from you.

33
Q

What is an S isomer?

A

A molecule that spins anticlockwise when the lowest priority functional group faces away from you.

34
Q

What is micibility?

A

The solubility of a liquid in another liquid.

35
Q

When is a solution formed?

A

When a substance disperses uniformly throughout another.

36
Q

What are three intermolecular forces?

A

Dispersion, dipole-dipole and hydrogen bonding.

37
Q

What is solvation?

A

The interaction between solute and solvent.

38
Q

What is hydration?

A

A solution where the solvent is water.

39
Q

What is the limitation of the Bohr model?

A

The Bohr model can explain the line spectra for H but not for any other atom.

40
Q

What did Bohr suggest about electrons? (2)

A

Electrons exist in discrete energy levels and energy is involved in moving an electron from one level to another.

41
Q

What are the letters used for electron orbitals (in order, give examples)?

A

S P D F (1s,2s,2p,3s,3p,3d,4s,4p,4d,4f)

42
Q

What is an electron shell?

A

A collection of orbitals with the same value for n.

43
Q

How many electrons can each shell hold?

A

n^2

44
Q

What shape are p-orbitals?

A

Dumbbell shaped

45
Q

What shape are d-orbitals?

A

4-leaf clover shaped apart from dz2 which has two lobes with a doughnut in the middle.

46
Q

What would happen if there was no restriction for the values of quantum numbers?

A

All electrons would revert to the ground state.

47
Q

How many electrons can be in each orbital?

A

2

48
Q

What is Hund’s rule?

A

For degenerate orbitals, the lowest energy is attained when the number of electrons with the same spin is maximised.

49
Q

What happens to first ionisation energy in each group?

A

First ionisation energy decreases with atomic number.

50
Q

What electrons are removed first?

A

Those that are in the least filled orbital with the largest quantum number

51
Q

Where are electrons added first?

A

The lowest quantum orbital that is partially filled.

52
Q

What is Coulomb’s law?

A

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
Q

What happens to attraction in a many electron atom?

A

Electrons are simultaneously attracted to the nucleus but repelled by other electrons.

54
Q

What is atomic radius?

A

Half of the distance between two identical nuclei that are chemically bonded.

55
Q

How is atomic radius effected in each group?

A

Atom radius increases from top to bottom. As we go down electrons have a higher chance of being further away from the nucleus.

56
Q

What happens to atomic radius in each period?

A

Atomic radius decreases from left to right. Increasing charge draws valence electrons closer.

57
Q

Define isoelectric series.

A

A group of icons containing the same number of electrons.

58
Q

What group has the lowest first ionisation energy?

A

Alkali metals

59
Q

What happens to first ionisation energy in each period?

A

First ionisation energy increases with atomic number.

60
Q

What are the three types of chemical bond?

A

Ionic, covalent and metallic

61
Q

What are ionic bonds?

A

Ionic bonds occur due to the differing bonds between adjacent ions.

62
Q

What happens in covalent bonding?

A

Two particles share electrons.

63
Q

What happens in metallic bonds?

A

In metallic bonds each atom is bonded to several neighbouring atoms and electrons are free to move around the structure.

64
Q

Which electrons are involved in bonding?

A

Valence electrons

65
Q

Which sub shells are full in an octet?

A

S and P

66
Q

What is a formal charge?

A

A formal charge is the charge a molecule would have if all the atoms in it were equally electronegative.

67
Q

What is a resonance Lewis structure?

A

Versions of the same molecule with different electron configurations.

68
Q

What is electron domain geometry?

A

The arrangement of electrons around a central atom

69
Q

What happens when all electron domains are bonds?

A

Molecular geometry = electron geometry

70
Q

What happens to bond angles when lone pairs of electrons are present?

A

The bond angles get smaller

71
Q

Which has a higher repulsion: non-bonding pairs or bonding pairs?

A

Non-bonding pairs

72
Q

What is a sigma bond?

A

A covalent bond where electrons are dispersed evenly.

73
Q

What is a pi-bond?

A

A bond with a sideways overlap of p-orbitals

CHE144 (4 decks)

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