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IMAT Chem > Chapter 2: Atomic Structure. Electron Configuration > Flashcards

Chapter 2: Atomic Structure. Electron Configuration Flashcards

1
Q

What does the relative atomic mass represent?

A

The average mass of an atom of the element.

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2
Q

What is the maximum number of electrons a single orbital can hold?

A

2 electrons.

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3
Q

What is the shape of an s orbital?

A

Spherical.

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4
Q

How many orbitals are present in the p subshell?

A

3 orbitals.

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5
Q

What is the maximum number of orbitals in a shell determined by?

A

n² (where n is the shell number).

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6
Q

How many orbitals does the d subshell have?

A

5 orbitals.

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7
Q

How many electrons can the p subshell hold?

A

6 electrons.

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8
Q

What is Hund’s third rule?

A

Electrons occupy separate orbitals with parallel spins to minimize energy.

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9
Q

What is the relationship between 4s and 3d orbitals?

A

They are close in energy.

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10
Q

What is particularly stable in electron configurations?

A

Half-filled and fully filled sub-levels.

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11
Q

How does electron configuration influence an element’s position on the Periodic Table?

A

It is based on the sub-level of highest energy in the ground-state atom.

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12
Q

Why does successive ionization energy increase?

A

Greater attractive force between protons and remaining electrons.

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13
Q

What are the three factors influencing ionization energy?

A

Nuclear charge

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14
Q

How does nuclear charge affect ionization energy?

A

Ionization energy increases with proton number.

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15
Q

What is the effect of electron distance from the nucleus on ionization energy?

A

Farther distance lowers ionization energy.

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16
Q

How does the shielding effect influence ionization energy?

A

More inner electron shells reduce ionization energy.

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17
Q

How does electron configuration minimize electron repulsion?

A

Electrons occupy separate orbitals.

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18
Q

What is the maximum number of electrons in an f subshell?

A

14 electrons.

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19
Q

What determines the energy levels of orbitals?

A

The principal quantum number (n) and subshell type.

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20
Q

Why are parallel spins favored in orbitals?

A

They lower energy by minimizing repulsion.

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21
Q

What is the shape of p orbitals?

A

Dumbbell-shaped.

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22
Q

How many p orbitals exist in a shell?

A

3 orbitals.

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23
Q

What is the maximum number of electrons in the n=3 shell?

A

18 electrons.

24
Q

Which subshell has 7 orbitals?

A

f subshell.

25
Q

How does ionization energy change across a period?

A

It generally increases.

26
Q

Why does ionization energy decrease down a group?

A

Increased shielding and electron distance.

27
Q

How many electrons can a d subshell hold?

A

10 electrons.

28
Q

What is the significance of a full d subshell?

A

Stability in the atom.

29
Q

Which orbitals are occupied first

A

4s or 3d?

30
Q

How are orbitals arranged within subshells?

A

They are filled to minimize energy.

31
Q

What is the maximum number of electrons in the n=2 shell?

A

8 electrons.

32
Q

What happens to electron repulsion in a full subshell?

A

It is minimized due to pairing.

33
Q

How many orbitals are there in an s subshell?

A

1 orbital.

34
Q

What subshells exist in the n=1 shell?

A

s subshell only.

35
Q

What is the principle behind the Aufbau process?

A

Electrons fill the lowest energy orbitals first.

36
Q

Which rule explains why no two electrons in an atom can have the same set of quantum numbers?

A

Pauli exclusion principle.

37
Q

What is the significance of orbital overlap in bonding?

A

It allows sharing of electrons.

38
Q

What factors determine the energy difference between orbitals?

A

Subshell type and nuclear charge.

39
Q

How does the shielding effect vary with atomic number?

A

It increases with more inner electron shells.

40
Q

How does the energy of 4p orbitals compare to 4s?

A

4p orbitals have higher energy.

41
Q

What is the shape of d orbitals?

A

Complex

42
Q

What rule governs the order of filling electron orbitals?

A

Aufbau principle.

43
Q

How many electrons can the 3p subshell hold?

A

6 electrons.

44
Q

What is the maximum number of orbitals in the n=4 shell?

A

16 orbitals.

45
Q

What explains the stability of noble gases?

A

Full outer electron shells.

46
Q

How does electron spin contribute to magnetic properties?

A

Unpaired spins create magnetic moments.

47
Q

What is the electron configuration of helium?

A

1s².

48
Q

How does the periodic table reflect electron configurations?

A

By grouping elements with similar outer electron configurations.

49
Q

Why does the first ionization energy of sodium drop compared to neon?

A

Sodium has an electron in a higher energy shell.

50
Q

What happens when an atom gains an electron?

A

It forms an anion.

51
Q

How does nuclear attraction affect ionization energy?

A

Greater attraction increases ionization energy.

52
Q

What is the electron configuration of carbon?

A

1s² 2s² 2p².

53
Q

How does ionization energy vary in a transition metal series?

A

It varies slightly due to d orbital filling.

54
Q

Which subshells are involved in the electron configuration of oxygen?

A

s and p subshells.

55
Q

What property of electrons leads to Hund’s rule?

A

Spin pairing energy.

56
Q

How do energy levels change as n increases?

A

They become closer together.

57
Q

What happens to atomic size as ionization energy increases?

A

It decreases.

IMAT Chem (9 decks)

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