Chapter 2: The Periodic Table Flashcards

1
Q

What are periods?

A
  • Rows

- Same principle energy level, n

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2
Q

What are groups?

A
  • Columns

- Same valence electron configuration

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3
Q

Where are the valence electrons of the lanthanide and actinide series?

A

s and f subshells

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4
Q

What are metals? Where are they found?

A
  • Shiny (lustrous, except for mercury), conduct electricity well, and are malleable and ductile;
    easily give up their electrons
  • Metals are found on the left side and middle of the Periodic Table.
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5
Q

What are non-metals? Where are they found?

A
  • Dull, poor conductors of electricity, and are brittle.

- Nonmetals are found on the right side of the Periodic Table.

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6
Q

What are metalloids? Where are they found?

A
  • Possess characteristics of both metals and non-metals and are found in a stair-step pattern starting with boron.
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7
Q

What is the effective nuclear charge (Zeff)?

A

The net positive charge experienced by electrons in the valence shell and forms the foundation for all periodic trends.

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8
Q

How does Zeff change from left to right in a period?

A

Increases

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9
Q

How does Zeff change from top to bottom in a group?

A

Little change

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10
Q

What is the atomic radius?

A

The size of a neutral element

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11
Q

How does the atomic radius change from left to right in a period?

A

Decreases

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12
Q

How does the atomic radius change from top to bottom in a group?

A

Increases

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13
Q

What is the ionic radius?

A

The size of a charged species

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14
Q

Are cations generally smaller or larger than their corresponding neutral atom? Where are they located?

A
  • Smaller

- Metals close to the metalloid line

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15
Q

Are anions generally smaller or larger than their corresponding neutral atom? Where are they located?

A
  • Larger

- Non-metals close to the metalloid line

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16
Q

What is the ionization energy?

A

The amount of energy (endothermic) necessary to remove an electron from the valence shell of a gaseous species

17
Q

How does the ionization energy change from left to right in a period?

A

Increases

18
Q

How does the ionization energy change from top to bottom in a group?

A

Decreases

19
Q

What happens if you remove a subsequent electron after attaining a noble gas-like configuration?

A

Removing the subsequent electron will cost much more energy

20
Q

What is electron affinity?

A

The amount of energy released (exothermic) when a gaseous species gains an electron in its valence shell

21
Q

How does the electron affinity change from left to right in a period?

A

Increases

22
Q

How does the electron affinity change from top to bottom in a group?

A

Decreases

23
Q

What is electronegativity?

A

measure of the attractive force of the nucleus for electrons within a bond

24
Q

How does the electronegativity change from left to right in a period?

A

Increases

25
Q

How does the electronegativity change from top to bottom in a group?

A

Decreases

26
Q

What oxidation state do alkali metals take?

A
  • +1

- To lose an electron and gain a noble gas-like configuration

27
Q

What oxidation state do alkali metals take?

A
  • +2

- Lose two electrons to achieve a noble gas-like configuration

28
Q

What oxidation state do chalcogens take?

A
  • -2 (metals) or +6 (non-metals)
29
Q

Which group is biologically important?

A

Chalcogens

30
Q

What oxidation state do halogens take?

A
  • -1

- Highest electronegativities

31
Q

Which groups has the highest ionization energies and virtually non-existent electronegativities?

A

Noble gases

32
Q

What explains the ability of transition metals to form colorful complexes with non-metals in solution?

A

The fact that they take on multiple oxidation states