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chemistry > chapter 7: ionic and metallic bonds > Flashcards

chapter 7: ionic and metallic bonds Flashcards

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1
Q

What are valence electrons?

A

Responsible for the chemical properties of atoms, and are those in the outer energy level.

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2
Q

What are core electrons?

A

those in the energy levels below (inner)

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3
Q

Atoms in the same column…

A
  • Have the same outer electron configuration.
  • Have the same valence electrons.
  • React similarly
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4
Q

What is the most amount of valence electrons that an atom can have?

A

8 valence electrons

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5
Q

The number of valence electrons are easily determined because…

A

It is the group number for a representative element
(ex.) Group 2A: Be, Mg, Ca, etc. have 2 valence electrons

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6
Q

What is the The Octet Rule?

A

in forming compounds, atoms tend to achieve a noble gas configuration; 8 in the outer level is stable

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7
Q

Octet rule for noble gases

A

Each noble gas (except He, which has 2) has 8 electrons in the outer level

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8
Q

Metals __ electrons to attain a noble gas configuration.

A

lose

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9
Q

Cations

A

positive ions

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10
Q

Anions

A

negative ions

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11
Q

Nonmetals __ electrons to attain noble gas configuration.

A

gain

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12
Q

Nonmetals make…

A

negative ions

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13
Q

Metals make…

A

positive ions

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14
Q

What are Halide ions?

A

ions from chlorine or other halogens that gain electrons

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15
Q

Anions and cations are held together by…

A

opposite charges

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16
Q

Ionic compounds are called…

A

Salts

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17
Q

Simplest ratio of elements in an ionic compound is called the…

A

Formula Unit

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18
Q

Ionic compounds are made from…

A
  • a CATION with an ANION
  • Or literally from a metal combining with a nonmetal
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19
Q

What is a chemical formula?

A

Shows the kinds and numbers of atoms in the smallest representative particle of the substance.

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20
Q

For an ionic compound, the smallest representative particle is called a:

A

Formula Unit

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21
Q

Properties of Ionic Compounds

A

Crystalline solids and high melting points

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22
Q

Crystalline solids

A
  • a regular repeating arrangement of ions in the solid
  • Ions are strongly bonded together.
  • Structure is rigid.
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23
Q

Coordination number

A

number of ions of opposite charge surrounding it

24
Q

Do Ionic Compounds conduct?

A

when a solid, they DO NOT conduct (they insulate) however when melted and dissolved in water they can conduct

25
Q

Metallic Bonds are…

A

How metal atoms are held together in the solid.

26
Q

Metals hold on to their valence electrons

A

Very weakly

27
Q

Metallic bonds are like

A

positive ions (cations) floating in a sea of electrons

28
Q

Sea of electrons

A

Electrons are free to move through the solid.
● Metals conduct electricity.

29
Q

Metals are…

A

Malleable and ductile

30
Q

Both malleability and ductility explained in terms of the…

A

mobility of the valence electrons

31
Q

Strong Repulsion

A

breaks a crystal apart, due to similar ions being next to each other.

32
Q

Crystalline structures of metal

A

If made of one kind of atom, metals are among the simplest crystals; very compact & orderly

33
Q

Body centered cubic

A

every atom (except those on the surface) has 8 neighbors
–Na, K, Fe, Cr, W

34
Q

Face centered cubic

A

every atom has 12 neighbors
–Cu, Ag, Au, Al, Pb

35
Q

Hexagonal close-packed

A

every atom also has 12 neighbors
–different pattern due to hexagonal
–Mg, Zn, Cd

36
Q

Alloys

A

mixtures of 2 or more elements, at least 1 is a metal

37
Q

How are alloys made

A

● made by melting a mixture of the ingredients, then cooling

38
Q

Why use alloys?

A

Properties are often superior to the pure element. (Stronger and last longer)

39
Q

How to find density

A

Mass divided by volume
d = M/V

40
Q

In ionic compounds…

A

electrons are fully transfered

41
Q

In covalent compounds

A

electrons are shared

42
Q

Polar covalent compounds…

A

are shared unevenly

43
Q

Pure covalent compounds…

A

are shared evenly

44
Q

Covalent compounds NEVER…

A

conduct electrivity

45
Q

Metallic ALWAYS

A

conduct electricity

46
Q

Metallic and ionic have very high…

A

melting and boiling points

47
Q

Covalent has

A

low melting and boiling points

48
Q

when creating a dot diagram

A

crisscross the charges

49
Q

ionic range

A

x > 1.7 (greater than 1.7)

50
Q

polar covalent range

A

less than or equal to 1.7 or greater than or equal to 0.3

51
Q

pure covalent range

A

less than 0.3

52
Q

pure covalent has

A

no charge

53
Q

polar covalent charge symbols

A

weird s with + or -

54
Q

ionic charge symbols

A

+ or -

55
Q

charges for the groups

A
  • group 1A: 1+
  • group 2A: 2+
  • group 3A: 3+
  • group 4A: 4+
  • group 5A: 3-
  • group 6A: 2-
  • group 7A: 1-
  • group 8A: 0
  • transition metals are group b

chemistry (6 decks)

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