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Chemistry I > Chapter 15 Test > Flashcards

Chapter 15 Test Flashcards

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1
Q

What are valence electrons?

A

The outermost electrons in an atom

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2
Q

How do valence electrons relate to bonding?

A

These are in the outermost shells of atoms, so they are usually the only electrons involved with bonding.

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3
Q

How do valences relate to group numbers? Is this true for all groups? Which groups is this true for?

A

They indicate the group number for groups 1A-8A, not the B groups

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4
Q

What is a cation?

A

A positively charged ion formed when an atom loses electrons

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5
Q

What kinds of elements are cations formed by and why do they do this?

A

Usually formed by metal atoms to achieve Noble Gas configurations and become stable

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6
Q

What kinds of elements are stable? What makes them stable?

A

Noble gases are most stable, outer subshells are full

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7
Q

What do all atoms want to do by common nature?

A

They want to adjust to achieve their lowest possible energy, their most stable energy state

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8
Q

What is an anion?

A

A negatively charged ion formed when an atom gains electrons

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9
Q

What kinds of elements are anions formed by and why do they do this?

A

Usually formed by nonmetal atoms to achieve Noble Gas configurations and become stable

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10
Q

What is a monatomic ion?

A

A single atom ion with only one kind of element

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11
Q

What is the suffix for monatomic ions?

A

-ide

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12
Q

What are some examples of monatomic ions and their new names?

A

O-oxygen
O-2-oxide

F-fluorine
F-1-fluoride

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13
Q

What is a polyatomic ion?

A

A group of different atoms with a charge. The group of atoms acts as a single unit.

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14
Q

What are the endings for polyatomic ions?

A

-ite and -ate

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15
Q

What is an example of a polyatomic ion?

A

CO2-carbon dioxide

CO3^-2-carbonate

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16
Q

Who proposed the Octet Rule?

A

Lewis

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17
Q

What is the Octet Rule?

A

Atoms react by changing the number of their electrons so as to acquire the stable electron structure of a noble gas

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18
Q

What is the Octet Rule really an explanation of?

A

Why atoms tend to form their respective types of ions

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19
Q

What is an ionic bond?

A

The force of attraction that bonds oppositely charged ions together

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20
Q

What kind of forces are present in ionic bonds?

A

electrostatic attractions

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21
Q

How does the ionic bonding relate to periodic trends?

A

Because nonmetals are smaller atoms with high EN and IE, they will pull off valence electrons from the metal atoms. they will gain electrons from metal atoms

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22
Q

What do ionic bonds form?

A

Ionic compounds

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23
Q

Why are all ionic compounds neutral?

A

The charges of anions plus the cation charges must equal 0.

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24
Q

What is a formula unit?

A

The lowest whole number ratio of ions in an ionic compound which keeps the identity of that ionic compound

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25
Q

What is a representative particle?

A

The smallest particle of a substance that keeps that substance’s identity

26
Q

What are the representative particles for elements and compounds?

A

Atoms are the RPs for elements

Formula units are the RPs for the ionic compounds

27
Q

What are some properties of ionic compounds?

A
  • composed of cations and anions

- electrically neutral charge, as cations and anions charges cancel each other

28
Q

When writing chemical formulas, which ion is writing first?

A

the cation

29
Q

What is the pattern structure of an ionic compound?

A

Crystal structure, repeating 3D pattern

30
Q

How do group B elements gain or lose electrons?

A

They lose outer electrons one at a time

31
Q

What is the coordination number? How does it relate to the atom’s crystal structure?

A

The number of oppositely charged ions touching a single ion. The shape of the crystal is determined by the ion’s charge and size.

32
Q

How does an ionic compound’s crystal strength relate to how it conducts electricity?

A

It must have a free movement of charge to conduct electricity. Crystal structure means that ions are locked into a fixed position and unable to move freely, thus do not conduct electricity.

33
Q

What is the ionic compound’s level of sturdiness?

A

They are brittle

34
Q

How are ionic compounds brittle?

A

When a force is applied to an ionic compound, like charges are forced together and in response, the like charges repel and the crystal shatters into smaller ones.

35
Q

What is the ionic compound’s level of solubility?

A

Readily soluable in water

36
Q

How are ionic compounds readily soluable in water?

A

They are easily dissolvable in water; they dissocate (separate into individual ions)

37
Q

What is the ionic compound’s property of melting point?

A

High melting point

38
Q

How do ionic compounds have a high melting point?

A

Determined by the strength of bonds, as bonds are strong, which raises the melting point, the stronger the bonds, the higher the melting point.

39
Q

What is the ionic compound’s flammability property?

A

not flammable

40
Q

How are ionic compounds not flammable?

A

They will not combust when put in a flame.

41
Q

What is the ionic compound’s conductor property?

A

They conduct in liquids

42
Q

How do ionic compounds conduct in liquids?

A

Liquid particles are more free to move around as more bonds break.

43
Q

Do ionic compounds conduct in solutions?

A

Yes

44
Q

Why do ionic compounds conduct in solutions?

A

Because ionic compounds dissocate when dissolved in water, the ions are free to move around and thus conduct electricity.

45
Q

What is a metallic bond?

A

The attraction between the free floating valence electrons and fixed positive nuclei of the metal atoms

46
Q

What are free floating valences called?

A

A sea of electrons

47
Q

Are metallic bonds malleable?

A

Yes

48
Q

How are metallic bonds malleable?

A

They are non-directional in their bonds

49
Q

How do metallic bonds work with many atoms?

A

The electrons in between can attract and slide over and attract to more than one atom

50
Q

Are metallic bonds ductile?

A

Yes

51
Q

What is an alloy?

A

A solution of metals

52
Q

Are metallic bonds good conductors?

A

Yes

53
Q

How are metallic bonds good conductors of heat and electricity?

A

The free floating valences cause them to slide over one another, attract to other nuclei and therefore transfer the heat and electricity from atom to atom

54
Q

What do metallic bonds conduct?

A

heat and electricity

55
Q

What are the two types of alloys?

A

substitutional alloys and interstitial alloys

56
Q

What are substitutional alloys?

A

Metal atoms in this alloy are the same size

57
Q

What are interstitial alloys?

A

Have metal atoms different in sizes at bonding, which causes for interstitial space, as the smaller atoms fit into these spaces

58
Q

Why are interstitial alloys more dense?

A

The smaller atoms fit into these interstitial spaces and cause for less room.

59
Q

How can you tell between hard and soft metals?

A

If an atom has 3 or more single “d” electrons, then they will bond and form a covalent network in addition to the metallic bonds, making them hard metals.

60
Q

What elements are the hard metals in the periodic table?

A

D3-D7 groups

Chemistry I (15 decks)

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