Brainscape's Knowledge GenomeTM

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


See full index

IMAT Chem > Chapter 4: Periodicity > Flashcards

Chapter 4: Periodicity Flashcards

1
Q

How are elements arranged in the Periodic Table?

A

By increasing atomic number.

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

What do the vertical columns in the Periodic Table represent?

A

Groups.

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

What do the rows in the Periodic Table represent?

A

Periods.

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

What trend is observed in atomic radii across a period?

A

Atomic radii decrease.

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

Why do atomic radii decrease across a period?

A

Increased nuclear charge pulls electrons closer.

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

What trend is observed in atomic radii down a group?

A

Atomic radii increase.

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

Why do atomic radii increase down a group?

A

More electron shells increase shielding.

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

How does the size of positive ions compare to their parent atoms?

A

Positive ions are smaller.

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

How does the size of negative ions compare to their parent atoms?

A

Negative ions are larger.

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

What is the trend in ionic radii for positive ions from Groups 1 to 14?

A

Ionic radii decrease.

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

What is the trend in ionic radii for negative ions from Groups 14 to 17?

A

Ionic radii decrease.

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

Why do ionic radii decrease across a period?

A

Increased nuclear charge.

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

What is the trend in ionic radii down a group?

A

Ionic radii increase.

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

What is the general trend of ionization energy across a period?

A

Ionization energy increases.

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

Why does ionization energy increase across a period?

A

Greater nuclear attraction makes electrons harder to remove.

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

What is the general trend of ionization energy down a group?

A

Ionization energy decreases.

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

Why does ionization energy decrease down a group?

A

Increased distance reduces nuclear attraction.

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

What is electronegativity?

A

An atom’s ability to attract electrons in a covalent bond.

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

What is the trend in electronegativity across a period?

A

Electronegativity increases.

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

What is the trend in electronegativity down a group?

A

Electronegativity decreases.

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

Which element has the highest electronegativity?

A

Fluorine (4.0).

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

Which element has the lowest electronegativity?

A

Caesium (0.7).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What happens to melting points down Group 1?

A

Melting points decrease.

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

Why do melting points decrease down Group 1?

A

Decreased attraction between delocalized electrons and ions.

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

What happens to melting points down Group 17?

A

Melting points increase.

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

Why do melting points increase down Group 17?

A

Stronger London dispersion forces.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

What is the general trend in melting points across a period?

A

Increase to Group 14

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

How does bonding change in Period 3?

A

Metallic → Giant covalent → Van der Waals forces.

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

What ions do Group 1 elements form?

A

Single positive ions (M+).

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

How do alkali metals react with water?

A

Form hydrogen and metal hydroxide.

31
Q

What ions do Group 17 elements form?

A

Single negative ions (M-).

32
Q

How do halogens react with Group 1 metals?

A

Form ionic halides.

33
Q

Why does chlorine displace bromide in reactions?

A

Chlorine has a stronger attraction for electrons.

34
Q

What type of molecules do halogens exist as?

A

Diatomic molecules (X2).

35
Q

What is the bonding nature of metallic oxides in Period 3?

A

Ionic and basic.

36
Q

What is the bonding nature of non-metallic oxides in Period 3?

A

Covalent and acidic.

37
Q

What are amphoteric oxides?

A

Oxides reacting with both acids and bases.

38
Q

Which Period 3 oxide shows amphoteric behavior?

A

Aluminium oxide.

39
Q

What holds Group 1 elements together in metallic structures?

A

Delocalized electrons and positive ions.

40
Q

What causes London dispersion forces to increase?

A

More electrons in a molecule.

41
Q

What trend occurs in metallic character across a period?

A

Decreases.

42
Q

What trend occurs in non-metallic character across a period?

A

Increases.

43
Q

Why do metallic structures have high melting points?

A

Strong metallic bonds.

44
Q

What determines bond type in covalent bonds?

A

Electronegativity difference.

45
Q

What type of bond forms if electronegativity difference is high?

A

Ionic bond.

46
Q

What type of bond forms if electronegativity difference is low?

A

Covalent bond.

47
Q

What group contains the most reactive metals?

A

Group 1.

48
Q

What group contains the most reactive non-metals?

A

Group 17.

49
Q

What happens to reactivity in Group 1 down the group?

A

Increases.

50
Q

What happens to reactivity in Group 17 down the group?

A

Decreases.

51
Q

What causes reactivity to increase in Group 1?

A

Easier electron loss.

52
Q

What causes reactivity to decrease in Group 17?

A

Harder electron gain.

53
Q

How does Group 1 store energy in reactions?

A

As exothermic heat.

54
Q

What happens to density down Group 1?

A

Density increases.

55
Q

What color are halogens in their elemental state?

A

Varies (e.g.

56
Q

What holds diatomic halogen molecules together?

A

Covalent bonds.

57
Q

What trend occurs in atomic mass across a period?

A

Atomic mass increases.

58
Q

How does electron shielding change down a group?

A

Increases.

59
Q

Why is shielding constant across a period?

A

Same principal quantum shell.

60
Q

What group does helium belong to?

A

Group 18 (Noble gases).

61
Q

What is a characteristic of noble gases?

A

Inert and unreactive.

62
Q

What phase are most Group 17 elements at room temperature?

A

Gases or liquids.

63
Q

What is the most abundant alkali metal?

A

Sodium (Na).

64
Q

What causes boiling points to increase in halogens?

A

Stronger intermolecular forces.

65
Q

What type of lattice does NaCl form?

A

Ionic lattice.

66
Q

Why does silicon have a high melting point?

A

Giant covalent structure.

67
Q

Why does argon have a low boiling point?

A

Weak van der Waals forces.

68
Q

What is the electron configuration of a sodium ion (Na+)?

A

1s² 2s² 2p⁶.

69
Q

What determines the strength of London dispersion forces?

A

Number of electrons.

70
Q

What defines Group 18 elements?

A

Full valence shell.

71
Q

How are period trends observed in electronegativity?

A

Left to right increase.

72
Q

What reaction product forms when halogens gain an electron?

A

Negative ions (X-).

73
Q

Why are alkali metals stored under oil?

A

To prevent reaction with air or water.

IMAT Chem (9 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions