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DAT General Chemistry > Course Saver General Chemistry > Flashcards

Course Saver General Chemistry Flashcards

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1
Q

What is the periodic trend for atomic radius?

A

Down and to the left. Towards Fr (In France you get Fat)

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2
Q

Why does the atomic radius get larger as you go to the left?

A

Effective Nuclear Charge = Zeff
- Gets larger as you go to the right, making the atomic radius smaller.

Zeff = Z - S
Z = nuclear charge
S = shielding electrons (core electrons/closer to the nucleus)
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3
Q

What is the radius of a neutral atom?

A

Atomic Radius

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4
Q

What is the radius of a charged species (ion)?

A

Ionic Radius

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5
Q

Is the ionic radius of a cation compared to its neutral species larger or smaller?

A

The cation is significantly smaller than its neutral species.

  • metals typically form cations
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6
Q

Is the ionic radius of a anion compared to its neutral species larger or smaller?

A

The anion is significantly larger than its neutral species.

  • non-metals typically form anions
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7
Q

Who typically forms cations?

A

Metals

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8
Q

Who typically forms anions?

A

Non-metals

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9
Q

What is an Isoelectronic Series?

A

When a group of atoms have the same number of electrons.

Ex: S2-, Cl-, Ar, K+, Ca2+
all isoelectronic to Ar

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10
Q

In an isoelectronic series, who has the smallest ionic radius?

A

The most positive ion, most protons.

  • If they all have the same number of electrons, the one with the most protons will pull the electrons in tighter, making it smaller.
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11
Q

In an isoelectronic series, who has the largest ionic radius?

A

The more negative ion, most electrons.

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12
Q

What is ionization energy?

A

The energy required to remove an electron.

  • Related to oxidation
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13
Q

What is the trend for Ionization Energy?

A

Up and to the right. Towards He.

  • Opposite of Atomic Radius
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14
Q

Why is the ionization energy endothermic?

A

Removing an electron requires energy.

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15
Q

Why does the ionization energy increase going to the right?

A

The effective nuclear charge (Zeff) increases to the right. Which makes it harder to remove an electron, requiring a greater ionization energy.

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16
Q

Why does the ionization energy increase going up the periodic table?

A

The atomic radius decreases. The electrons are closer to the nucleus, making them harder to remove.

17
Q

Why are the alkali metals so reactive with H2O?

A

Because they have such low ionization energies, so they get oxidized really easily.

18
Q

What are the 2 exceptions to the ionization energy rule?

A

B & O have slightly lower energies (same goes for Al & S

  • If Boron loses an electron then he will have a full shell.
  • If Oxygen loses an electron then it will have a 1/2 full valence shell.
19
Q

What is the energy change associated with gaining an electron?

A

Electron Affinity

  • Exact opposite of Ionization Energy
  • Associated with reduction
20
Q

Why is Electron Affinity typically exothermic?

A

Gaining an electron is energetically favorable, because it lowers the atoms energy.

21
Q

What is the periodic trend for Electron Affinity?

A

It increases as you go to the right.

- It becomes more exothermic or negative.

22
Q

What are the exceptions to the Electron Affinity trend?

A
  • Noble Gases: have a filled octet, they don’t want another electron. They have a positive electron affinity & are endothermic.
  • Group 2 & 15 (Be & N columns): for the same reason as the ionization energy exception (full or 1/2 full sub-shells). They are either endothermic or only slightly exothermic.
23
Q

What is the periodic trend for Electronegativity?

A

Up and to the right. Towards F.

24
Q

What is electronegativity?

A

Measure of how close an atom pulls the shared electrons in a covalent bond to them.

25
Q

The most polar bond between 2 atoms is the one that has the greatest …

A

difference in electronegativity

Ex: C-F > C-O > C-N
Most polar/ greatest diff. in electronegativity.

26
Q

Which of the periodic trends is related to covalent bonding?

A

Electronegativity

27
Q

Which of the periodic trends is related to ionic bonding?

A

Ionization Energy & Electron Affinity

DAT General Chemistry (1 decks)

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