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Chemistry > Topic 3 The Periodic Table > Flashcards

Topic 3 The Periodic Table Flashcards

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1
Q

What is the aim of studying the periodic table?

A

To revise nomenclature, chemical calculations, trends in the periodic table, groups of elements, determine electron configurations, and calculate electrons in ions.

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2
Q

What are the columns of the periodic table called?

A

Groups.

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3
Q

What are the horizontal rows of the periodic table called?

A

Periods.

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4
Q

What is the atomic radius?

A

The total distance from the nucleus of an atom to the outermost orbital of its electron.

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5
Q

What trend occurs in atomic radius within a group as you move from top to bottom?

A

Atomic radius increases.

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6
Q

What causes the increase in atomic radius down a group?

A

Increase in the principal energy number (n) of the outer electrons.

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7
Q

What trend occurs in atomic radius within a period as you move from left to right?

A

Atomic radius decreases.

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8
Q

What is the effective nuclear charge (Zeff)?

A

The net positive charge attracting an electron in an atom.

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9
Q

How is effective nuclear charge approximated?

A

Zeff = Z – S, where Z is atomic number and S is the number of shielding electrons.

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10
Q

What is electronegativity?

A

The measure of an atom’s ability to attract electrons in a chemical compound.

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11
Q

Which element is the most electronegative?

A

Fluorine (F).

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12
Q

What trend occurs in electronegativity within a period as you move from left to right?

A

Electronegativity increases.

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13
Q

What trend occurs in electronegativity down a group?

A

Electronegativity decreases.

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14
Q

What is the octet rule?

A

Stability comes from having a full outer shell of electrons, typically eight.

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15
Q

What are alkali metals?

A

Group 1 elements with one electron in the outermost shell.

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16
Q

What is the electron configuration of Lithium (Li)?

A

1s² 2s¹.

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17
Q

What is the electron configuration of Cesium (Cs)?

A

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ 6s¹.

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18
Q

What are alkaline earth metals?

A

Group 2 elements with two electrons in their outer valence shell.

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19
Q

What is the typical oxidation state of transition metals?

A

They can exist in a range of oxidation states from +1 to +7.

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20
Q

What are the elements in Group 15 called?

A

Pnictogens.

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21
Q

What are the elements in Group 16 called?

A

Chalcogens.

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22
Q

What are the elements in Group 17 called?

A

Halogens.

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23
Q

What is the ability of an atom to withdraw a shared pair of electrons called?

A

Electropositivity.

24
Q

Does Mg or Mg²⁺ have a smaller radius?

A

Mg²⁺.

25
Q

What is the Aufbau principle?

A

Electrons occupy the lowest energy orbitals wherever possible.

26
Q

What is the Pauli exclusion principle?

A

No two electrons with the same spin can occupy the same orbital.

27
Q

What is Hund’s rule?

A

Electrons will occupy degenerate orbitals singly before pairing up.

28
Q

What is the electron configuration notation for Magnesium?

A

[Ne] 3s².

29
Q

What is a semiconductor?

A

Materials like silicon and germanium that partially conduct and partially insulate.

30
Q

What is the electron configuration for Neon?

A

1s² 2s² 2p⁶

31
Q

What is the electron configuration for Fluorine?

A

1s² 2s² 2p⁵

32
Q

What is the electron configuration for Beryllium?

A

1s² 2s²

33
Q

What is the electron configuration for Sodium?

A

1s² 2s² 2p⁶ 3s¹

34
Q

What is the challenge electron configuration for Zinc?

A

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰

35
Q

What is ionisation energy?

A

The minimum energy required to remove an electron from the ground state of the isolated gaseous atom or ion.

36
Q

What is the first ionisation energy (I₁)?

A

The energy required to remove one electron from a gaseous neutral atom.

37
Q

What is the second ionisation energy (I₂)?

A

The energy required to remove a second electron from a gaseous ion.

38
Q

True or False: The greater the magnitude of ionisation energy, the easier it is to remove the electron.

A

False

39
Q

Define a cation.

A

A positive ion that results from losing electrons.

40
Q

Define an anion.

A

A negative ion that results from gaining electrons.

41
Q

What is the ion symbol for sodium as a cation?

A

Na⁺

42
Q

What is the ion symbol for magnesium as a cation?

A

Mg²⁺

43
Q

What is the ion symbol for oxygen as an anion?

A

O²⁻

44
Q

What is the ion symbol for chlorine as an anion?

A

Cl⁻

45
Q

Fill in the blank: Ions can exist as _______ if they lose electrons.

A

+1, +2, or +3

46
Q

Fill in the blank: Ions can exist as _______ if they gain electrons.

A

-1, -2, or -3

47
Q

What do Group One elements do to form ions?

A

Lose one electron to become +1.

48
Q

What do Group Two elements do to form ions?

A

Lose two electrons to become +2.

49
Q

What do Transition Metals typically do to form ions?

A

Can vary but can be either +1, +2, or +3.

50
Q

What do Group Three (13) elements do to form ions?

A

Lose three electrons to become +3.

51
Q

What do Group Five (15) elements do to form ions?

A

Gain three electrons.

52
Q

What do Group Six (16) elements do to form ions?

A

Gain two electrons.

53
Q

What do Group Seven (17) elements do to form ions?

A

Gain one electron.

54
Q

Fill in the blank: Group Eight (18) elements are _______ and do not gain or lose electrons.

A

stable

55
Q

Challenge: What is an example of an ionic compound formed between Group One and the halogens?

A

NaCl (sodium chloride)

56
Q

Challenge: Provide an example of an ionic compound formed between Group Two and a Group 16 element.

A

CaO (calcium oxide)

57
Q

Challenge: Give an example of an ionic compound formed between Fe³⁺ and a Group 17 element.

A

FeCl₃ (iron(III) chloride)

Chemistry (6 decks)

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