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CHE 1211 Gen > Ch. 7 Electron Configuration and Periodic Table > Flashcards

Ch. 7 Electron Configuration and Periodic Table Flashcards

1
Q

Based on the type of subshell containing the outermost electrons, elements can be divided into ____?

A

Categories

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2
Q

What are the 6 categories that elements are divided into on the periodic table?

A
  1. Main Group Elements
  2. Noble Gases
  3. Transition Metals
  4. Volatile Metals
  5. Lanthanides
  6. Actinides
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3
Q

What part of the periodic table makes up the main group elements?

A

Groups 1A-7A

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4
Q

What part of the periodic table makes up Noble Gases?

A

Group 8A

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5
Q

What part of the periodic table makes up Transition Elements?

A

Group 3-11

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6
Q

What part of the periodic table makes up Volatile Metals?

A

Group 12

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7
Q

What part of the periodic table makes up the Lanthanides and Actinides?

A

Floating grid

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8
Q

The key to periodicity is____.

A

Atomic Number

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9
Q

Elements in a column of the modern periodic table have very similar ____ properties.

A

Chemical

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10
Q

An outer electron feels an ____ to the nucleus and a ____ to an inner electron. This is known as What?

A

Attraction
Repulsion
Shielding or Screening

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11
Q

Core electrons are most effective at shielding ___ ___.

A

Valence Electrons

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12
Q

The number of protons and the number of valence electrons increase from ___ to ____. Therefore so does the Zeff.

A

Left to right

Across a period

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13
Q

This is the magnitude of positive charge that is “felt” by a shielded electron. It is always positive.

A

Effective Nuclear Charge, Zeff

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14
Q

Because of shielding the effective nuclear charge is ___ than the actual nuclear charge.

A

less

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15
Q

Each step down in a group represents what in regards to the Zeff.

A
  1. a large increase in the nuclear charge, Z

2. an additional shell of core electrons to shield the valence electrons from the nucleus.

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16
Q

What are the two ways to define atomic radius?

A
  1. Metallic radius

2. Covalent radius

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17
Q

This is the atomic radius that is half the distance between the nuclei of two adjacent, identical metal atoms.

A

Metallic Radius

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18
Q

This is the atomic radius that is half the distance between adjacent, identical nuclei in a molecule.

A

Covalent Radius

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19
Q

What are the 2 atomic radius rules?

A
  1. The atomic radius increases from top to bottom in a group.
  2. It decreases as we move across a period from left to right.
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20
Q

This is the minimum energy required to remove an electron from an atom in the gas phase. It is a measure of the strength from with which an atom holds onto its electrons.

A

Ionization Energy (IE)

21
Q

The first ionization energy is the removal of the most ____ held electron.

A

loosley

22
Q

The first ionization energy is the removal of the most ____ held electron.

A

loosley

23
Q

What are the 2 Ionization Energy rules?

A
  1. The ionization energy decreases down a group.

2. It increases from left to right.

24
Q

___ electrons are generally more strongly bound from left to right in a period.

A

Valence

25
Q

This is the energy released when an atom is the gas phase accepts an electron, so it is the negative of the enthalpy change, delta H.

A

Electron Affinity

26
Q

What are the rule of electron Affinity?

A

It increases from left to right across a period, because it is easier to add negatively charged electrons as the positive charge of the elements nucleus increases.

27
Q

Which 2 groups do not form stable negative ions?

A

2A- alkali earth metals

8A- Noble Gases

28
Q

It is important to write out orbital diagrams for the valence electrons in which type of problems?

A

Electron Affinity.

29
Q

It is more difficult in Electron Affinity to add an electron to a ____ occupied orbital than to an empty one.

A

partially

30
Q

These are characteristics of?

  1. Shiny, lustrous, and malleable
  2. Good conductors of heat and electricity
  3. Low ionization energies (so they easily lose their valence electrons to form cations)
  4. Form Ionic compounds with chlorine (metal chlorides)
  5. Form basic compounds with oxygen (metal oxides)
A

Metals

31
Q

These are characteristics of?

  1. Vary in color and lack shiny appearance. Dull
  2. Brittle rather than malleable
  3. Poor conductors of heat and electricity
  4. Form acidic, molecular compounds with oxygen.
  5. Have high electron affinities (commonly form anions when they accept electrons)
A

Non-Metals

32
Q

What are the 2 ionization energy rules of metals?

A
  1. IE decreases going down a group

2. IE increases from left to right

33
Q

What are the 2 rules of metallic characteristics?

A
  1. Increase as you go down a group

2. Decrease from left to right in a period

34
Q

The valence electron configurations of Noble Gases are extraordinarily ____.

A

Stable

35
Q

Other main group elements tend to either ___ or ___ a electrons to acheive the same number of electrons as the nearest noble gas.

A

Lose or Gain

36
Q

Species with identical electron configurations are called what?

A

Isoelectronic

37
Q

To write the electron configuration of an ion formed by a main group element, you must…

A
  1. Write the configuration for the atom

2. Add or remove the appropriate number of electrons

38
Q

An atom always loses electrons first from the shell with the highest value of ___. Therefore valence electrons are always lost first.

A

n

39
Q

When an atom gains or loses one or more electrons to become an ion, its radius changes.

A

Ionic Radius

40
Q

The ionic radius affects the ___ and ___ chemical properties of ionic compounds.

A

Physical and Chemical

41
Q

When an atom loses electrons and becomes a cation, its radius ____.

A

Decreases

42
Q

____ electrons lead to:
A reduction in electron-electron repulsion and
A reduction in shielding of the valence electrons and
A higher Zeff.

A

Fewer

43
Q

A substantial ____ in radius occurs when all of an atoms valence electrons are removed. This is the case with ions of most main group elements which are isoelectronic.

A

decrease

44
Q

When an atom gains one or more electrons and becomes and anion its radius ____.

A

increases

45
Q

____ electrons leads to:
Increased electron-electron repulsion and therefore
A higher degree of shielding of the valence electrons and
Lower Zeff.

A

Additional

46
Q

Ionic radius ____ going down a group as n increases.

A

increases

47
Q

This is a series of two for more species that have identical electron configurations but different nuclear charges.

A

isoelectronic series

48
Q

What is an example of an isoelectronic series?

A

O^2, F- and Ne. they all have 10 electrons

49
Q

In an isoelectronic series, the species with the ____ nuclear charge will have the largest radius. And species with the ____ nuclear charge will have the smallest radius.

A

smallest

largest

CHE 1211 Gen (8 decks)

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