Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > Chapter 1 > Flashcards

Chapter 1 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

What 3 things make up atoms?

A

Protons, neutrons and electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What charge do electrons have?

A

-1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What do electrons wizz round the nucleus in?

A

Orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What takes up most of the volume of the atom?

A

The orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Where is most of the mass of the atom located?

A

In the nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is located in the nucleus?

A

Protons and neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What is the relative mass of a proton?

A

1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is the relative charge of a proton?

A

+1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What is the relative mass of a neutron?

A

1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is the relative charge of a neutron?

A

0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is the relative mass of an electron?

A

0.0005

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What does the mass number tell you?

A

The number of protons and neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What does the atomic number tell you?

A

The number of protons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What does it tell you if 2 elements have the same atomic number?

A

They are isotopes of each other

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

For neutral atoms, what does the number of protons equal?

A

The number of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What do ions have different numbers of?

A

Protons and electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What is the relative atomic mass?

A

The weighted mean mass of an element compared to 1/12th of the mass of a carbon-12 atom.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What is the Relative isotopic mass?

A

The mass of an atom of an isotope compared with 1/12th of the mass of carbon-12.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What is the relative molecular mass?

A

The average mass of a molecule or formula unit, compared to 1/12th of the mass of carbon-12.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

When is the relative molecular mass used?

A

When referring to simple molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

When is the relative formula mass used?

A

For ionic or giant covalent compounds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

How can the relative atomic mass be worked out from isotopic abundances?

A
  • Multiply each relative isotopic mass by it % abundance and add up the results
  • Divide by 100
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What is mass sprectra produced by?

A

Mass sprectrometers

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What are mass spectrometers?

A

Devices which are used to find out what samples are made up of by measuring the masses of their components

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

What useful thing can mass sprectrometers show us?

A

The relative isotopic masses and abundances of different elements.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

How do you work out the relative atomic mass from a mass spectrometer graph?

A
  • Multiply each relative isotopic mass by its relative isotopic abundance and add up the results
  • Divide the result by the sum of the isotopic abundances
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

How can mass spectrometry help identify compounds?

A

The molecular ion peak will tell you the molecular mass of the compound

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

What are electron shells made up of?

A

Shells and orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Do shells closer or further away from the nucleus have higher energy levels?

A

Shells further away from the nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What do subshells contain?

A

Orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

What can 1 orbital hold up to?

A

2 electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

How many orbitals does an ‘s’ subshell contain?

A

1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

How many orbitals does an ‘p’ subshell contain?

A

3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

How many orbitals does an ‘d’ subshell contain?

A

5

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

How many orbitals does an ‘f’ subshell contain?

A

7

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

How many electrons can an ‘s’ subshell contain?

A

2

37
Q

How many electrons can an ‘p’ subshell contain?

A

6

38
Q

How many electrons can an ‘d’ subshell contain?

A

10

39
Q

How many electrons can an ‘f’ subshell contain?

A

14

40
Q

What is an orbital?

A

The bit of space that an electron moves in?

41
Q

What is ‘spin-pairing’?

A

When the electrons in each orbital have to spin in opposite directions

42
Q

What shape are ‘s’ orbitals?

A

Spherical

43
Q

What shape are ‘p’ orbitals?

A

Dumbell shape

44
Q

What angle are 3 p-orbitals at to each other?

A

90 degree angles

45
Q

What subshells do electrons fill up first?

A

The lowest energy subshells

46
Q

What is the only exception in the subshell energy trend?

A

The 4s subshell has less energy than the 3d subshell

47
Q

What fills up first, the 4s subshell or the 3d subshell?

A

The 4s subshell

48
Q

Do electrons fill orbitals singly before they pair up?

A

Yes

49
Q

What do the s-block elements have an outer shell electronic configuration of?

A

S1 or S2

50
Q

What do the p-block elements have an outer shell electronic configuration of?

A

S2P1 to S2P6

51
Q

How do you work out the electronic configuration of an ion?

A

Write the elctronic configuration of the atom, then add or remove electrons to or from the highest energy subshell

52
Q

Why do chronium and copper donate one of their 4s electrons to the 3D subshell?

A

Because they are more stable with a full or half full d-subshell

53
Q

What is Electromagnetic radiation?

A

Energy that’s transmitted as waves

54
Q

What happens to the frequency of the radiation as you go along the Electromagnetic spectrum?

A

It increases

55
Q

In ground state, where do atoms have their electrons?

A

In their lowest possible energy levels

56
Q

If an atom’s electrons take in energy from their surroundings, what can happen?

A

The electrons can move to higher energy levels, further from the nucleus

57
Q

What are electrons said to be at higher energy levels?

A

More ‘excited’

58
Q

When electrons drop energy levels, what do they release?

A

Energy, which has fixed values

59
Q

What does an emission spectrum show?

A

The frequencies of light emitted when the electrons drop down energy levels.

60
Q

Why is the emission spectrum for each element unique?

A

Because each element has a different electron arrangement, so the frequencies of radiation absorbed and emitted are different

61
Q

Where is the only place electrons can exist?

A

In fixed orbits, or shells

62
Q

What does each quantum shell have a fixed value of?

A

Energy

63
Q

When an electron moves between shells, what is emitted or destroyed?

A

Electromagnetic radiation

64
Q

As the energy of shells is fixed, what does this mean about the frequency?

A

It has a fixed value

65
Q

What is the first ionisation?

A

The energy needed to remove 1 electron from each atom in 1 mole of gaseous atoms to form 1 mole of gaseous 1+ ions

66
Q

What is the equation for the 1st ionisation of oxygen?

A

O –> 0+ + e-

67
Q

What are the 3 main factors that affect ionisation energy?

A

Nuclear charge, electron shells, shielding

68
Q

How does nuclear charge affect ionisation energy?

A

The more protons, the more positively charged the nucleus is, so the stronger the attraction to the electrons

69
Q

How does electron shell effect ionisation energy?

A

Attraction falls off rapidly with distance. An electron in a shell close to a nucleus will be much more strongly attracted to the nucleus than one far away

70
Q

How does shielding effect ionisation energy?

A

As the number of electrons between the outer electrons and the nucleus increases, the outer electrons feel less attraction to the nucleus

71
Q

What does a high ionisation energy mean?

A

There is a strong attraction between the electron and the nucleus, so more energy is needed to overcome the attraction and remove the electron

72
Q

What happens to the 1st ionisation energy as you go down a group?

A

It decreases

73
Q

Why does the 1st ionisation energy decrease as you go down a group?

A
  • More shielding

- More shells

74
Q

What is the 2nd ionisation energy?

A

The energy needed to remove an electron from each ion in 1 mole of gaseous 1+ ions to form 1 mole of gaseous 2+ ions.

75
Q

What is the equation for the 2nd ionisation energy of oxygen?

A

O+ —> O2+ + e-

76
Q

What happens to the values of ionisation energies as more electrons are removed?

A

They increase

77
Q

Why does the value of the ionisation energies increase as more electrons are removed?

A

The ion becomes increasingly positive, so there’s less repulsion amongst the remaining electrons

78
Q

What are the big jumps in successive ionisation energies?

A

When a new shell is being broken into, as an electron is being removed from a shell close to the nucleus

79
Q

What happens to the atomic radius as you go across a group?

A

The atomic radius decreases

80
Q

What is the general trend for ionisation energy across a period?

A

Ionisiation energy generally increases across a period

81
Q

Why does ionisation energy generally increase across a period?

A

Stronger nuclear attraction due to more protons, and all the electrons are roughly at the same energy level, so there’s little shielding added

82
Q

Why is there small drops in ionisation energy across a period as you go from group 2 to group 3?

A

e.g. Aluminium’s outer electron is in a 3p orbital rather than a 3s orbital. The 3p orbital has slightly higher energy than the 3s orbital, so the electron is found further from the nucleus. The 3p orbital has additional shielding from the 3s electrons

83
Q

What is the drop in ionisation energy from group 5 to 6 across a period due to?

A

Electron repulsion:
Elements with singly fulled or full subshells are more stable than those with partially filled subshells, so have higher ionisation energies

84
Q

Why is it easier to remove electrons from shared orbitals?

A

Because there is repulsion between the 2 electrons in the orbital

85
Q

For metals, how does melting and boiling points change as you go across a period?

A

They increase

86
Q

Why do melting and boiling points increase as you go across a period for metals?

A

Metallic bonds get stronger because:

  • Metals have an increasing number of delocalised electrons
  • Metals have decreasing radius
87
Q

Why do the elements with strong giant covalent lattices have a high melting/boiling point?

A

They have strong covalent bonds, meaning a lot of energy is required to break them

88
Q

Why do elements with simple molecular structures have low melting/boiling points?

A

London forces are weak and easily overcome, so these elements have low melting/boiling points.

89
Q

Why do the noble gases have the lowest melting/boiling points?

A

Because they exist as individual atoms, resulting in weak London forces

Chemistry (25 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions