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Chemistry > Week 3 > Flashcards

Week 3 Flashcards

1
Q

Name two properties of metals that are about electrons and IE.

A
  1. Small ionization energy

2. Tend to lose electrons and become cations.

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2
Q

Name four properties of nonmetals related to electrons and electronegativity.

A
  1. Low energy open orbitals
  2. Gain electrons and become anions.
  3. Large EN (X)
  4. Have a high IE
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3
Q

What is the driving force of atoms?

A

They all want to have low energy.

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4
Q

What do atoms of the main group elements want to be isoelectronic with?

A

Elements of the noble gases. This group of elements that want to be isoelectronic with includes groups 1-2 and 13-18.

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5
Q

What does isoelectronic mean?

A

An atoms has the same electron configuration as a noble gas.

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6
Q

What do alkaline metals (group 1) prefer to do?

A

They prefer to lose an electron and become isoelectronic with noble gases. [monoatomic cations.]

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7
Q

What do alkaline earth metals (group 2) need to do?

A

Needs to loose two electrons to become isoelectronic with the noble gases.

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8
Q

What do halogens (group 17) have to do to be isoelectronic?

A

Have to gain electrons to become isoelectronic and become monoatomic anions.

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9
Q

What does column/group 16 have to do to become isoelectronic?

A

Gain two electrons, having a charge of -2.

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10
Q

What is the special case with aluminum?

A

It has to loose three electrons to become isoelectronic.

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11
Q

What do cations have?

A

High energy electrons that they tend to lose.

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12
Q

What are the two divides of compounds that define electron ownership?

A
  1. oxidation states

2. formal charge

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13
Q

Define oxidation states

A

Accounting for electrons when naming ionic compounds. Basically an electron accounting system. This is assuming all bonds a ionic, even ones that are not.

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14
Q

Hydroxide

A

(OH)-1

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15
Q

Carbonate

A

(CO3)-2

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16
Q

Bicarbonate (aka hydrogen carbonate)

A

(HCO3)-1

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17
Q

Cyanide

A

(CN)-1

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18
Q

Sulfate

A

(SO4)-2

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19
Q

Sulfite

A

(SO3)-2

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20
Q

Nitrate

A

(NO3)-1

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21
Q

Nitrite

A

(NO2)-1

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22
Q

Phosphate

A

(PO4)-3

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23
Q

Acetate

A

(C2H3O2)-1 or 0Ac(-)

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24
Q

Hydronium

A

(H3O)+1

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25
Q

Ammonium

A

(NH4)+1

26
Q

Rules for oxidation states

A

(In this order)

  1. The oxidation states of the atoms in an element (pure elements) are all zero.
  2. Fluorine is always assigned an oxidation number of -1.
  3. Group 1A metals are +1, Group 2A metals are +2, and aluminum is +3.
  4. H is +1 when bonded to non-metals. H is –1 when bonded to most metals.
  5. Oxygen is assigned an oxidation number of –2.
  6. Group 7A elements (halogens) are assigned an oxidation number of -1.
27
Q

Covalent bonds

A

Two atoms that have the same type of element and that share electrons equally.

28
Q

Polyatomic ions

A

Groups of charged covalently bound atoms.

29
Q

Monatomic ion

A

One atom with a charge

30
Q

Ionic compounds

A

A combinations with more than one cation and more than one anion. Usually a bond between a metal and a nonmetal.

31
Q

Rules for naming monatomic cation

A

Name doesn’t change

32
Q

Monatomic cation

A

Single atom where electrons are lost.

33
Q

Monatomic anion

A

Single atom where electrons are gained.

34
Q

Rules for naming monatomic anion

A

Ending changes to -ide.

35
Q

Where are electrons usually taken from?

A

Metals, then given to nonmetals.

36
Q

What are the rules for naming metals and late metals in ionic compounds.

A

Have to tell what the oxidation state is. This is told by Roman numerals. Zinc and silver are exceptions.

37
Q

Where are covalent bonds seen?

A

Normally with atoms of similar electronegativity. These don’t contain metallic elements (there are a few exceptions) and form between nonmetals.

38
Q

Name properties of ionic bonds

A
  1. When some atoms are negative and some are positive.
  2. These are solid and are non-directional (they don’t know what atoms they are bonded to.)
  3. Electrons are taken from another atom.
39
Q

Molecular compound

A

Is directional and shares electrons.

40
Q

Nonpolar covalent bonds

A

When the electronegativity between atoms is around zero.

41
Q

Polar covalent bond

A

When the EN is more than 0.4.

42
Q

What happens when metal bonds with a nonmetal?

A

The result is an ionic bond.

43
Q

Rules for naming ionic compounds

A
  1. For monatomic anion, the ending changes to -ide. For monatomic cations, the ending does not change.
  2. If an ionic compound is not in Group IA or Group 2A, and is a metal or a late metal, then the name must contain a Roman numeral. Zinc and silver are exceptions.
44
Q

Rules for naming covalent and molecular compounds

A
  1. Without hydrogen, the elements are ranked by their electronegativity. (less EN, more EN.)
  2. The electronegative elements is seen as an anion, even when it isn’t one.
  3. The suffix is changed to -ide.
  4. Each element gains a greek prefix to tell how many atoms there are of each element.
45
Q

What are the three branches of naming rules?

A
  1. Ionic compounds
  2. Covalent compounds
  3. Acids
46
Q

What do molecular compounds contain?

A

Covalent bonds

47
Q

Binary covalent bonds

A

Have two types of elements

48
Q

1 atom

A

mono => not used for first atom in formula

49
Q

2 atoms

A

di

50
Q

3 atoms

A

tri

51
Q

4 atoms

A

tetra

52
Q

5 atoms

A

penta

53
Q

6 atoms

A

hexa

54
Q

7 atoms

A

hepta

55
Q

8 atoms

A

octa

56
Q

9 atoms

A

hona

57
Q

10 atoms

A

deca

58
Q

Formula mass

A

Ratio between a mole of the compound and the weight of a compound.

59
Q

Molecular mass

A

finding the mass of a compound

60
Q

Two types of ionic bonds.

A

1) Group 1A and 2A with 6A and 7A.

2) Transition metals with nonmetals.

61
Q

Types of covalent bonds.

A

Between anything else outside of the ionic bonds.

Chemistry (9 decks)

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