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Chemistry > Chemistry (Chapter 7) > Flashcards

Chemistry (Chapter 7) Flashcards

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1
Q

S1) How can you determine the number of valence electrons in an atom of a representative element?

A

Look at its group number.

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2
Q

S1) Atoms of which elements tend to gain electrons? Atoms of which elements tend to lose electrons?

A

Atoms of metallic elements lose their valence electrons, leaving a complete octet in the lowest energy level. Atoms of some nonmetallic elements gain electrons to achieve a complete octet.

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3
Q

S1) How do cations form?

A

An atom’s loss of valence electrons produces a positively charged cation.

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4
Q

S1) How do anions form?

A

The gain of electrons by a neutral atom produces negatively charge anion.

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5
Q

S1) How do you describe the electrical charge of an ionic compound?

A

Ionic compounds are electrically neutral.

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6
Q

S1) What properties characterize ionic compounds?

A

Most ionic compounds are crystalline solids at room temperature, and they generally have high melting points. Ionic compounds can conduct an electric current when melted or dissolved in water.

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7
Q

S1) How do chemists model the valence electrons in metal atoms?

A

The valence electrons of metal atoms can be modeled as a sea of electrons.

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8
Q

S1) How can you describe the arrangements of atoms in metals?

A

Metal atoms are arranged in very compact and orderly patterns.

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9
Q

S1) Why are alloys more useful than pure metals?

A

Alloys are important because their properties are often superior to those of their component elements.

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10
Q

How is an anion produced?

A

It is produced when an atom gains one or more valence electrons.

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11
Q

What is a valence electron?

A

An electron in the highest occupied energy level of an atom.

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12
Q

What is electron dot structure?

A

A notation that depicts valence electrons as dots around the atomic symbol of the element; the symbol represents the inner electrons and atomic nucleus; also called Lewis dot structure.

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13
Q

What is the octet rule?

A

Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas, usually eight valence electrons.

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14
Q

What is the halide ion?

A

A negative ion formed when a halogen atom gains an electrons.

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15
Q

What is an ionic compound?

A

A compound composed of positive and negative ions.

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16
Q

What is an ionic bond?

A

The electrostatic attraction that binds oppositely charged ions together.

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17
Q

What is a chemical formula?

A

An expression that indicates the number and type of atoms present in the smallest representative unit of a substance.

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18
Q

What is a formula unit?

A

The lowest whole-number ratio of ions in an ionic compound.

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19
Q

What is a coordination number?

A

The number of ions of opposite charge that surround each ion in a crystal.

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20
Q

Elements within the same group of the periodic table behave the same because they have the same number _____.

A

Valence Electrons.

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21
Q

______ on the periodic table indicates how many valence electrons that element has.

A

Group number.

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22
Q

Diagrams that show valence electrons as dots.

A

Electron Dot Structure.

23
Q

States that in forming compounds, atoms tend to achieve the electron configuration of a noble gas.

A

Octet Rule

24
Q

The cations of group 1A always have what charge?

A

Positive one.

25
Q

What are positively charged ions called?

A

cations

26
Q

What are negatively charged ions called?

A

anions.

27
Q

What are produced when elements in group 7A gain an electron?

A

Halide ions.

28
Q

What is the charge of cation transition metals?

A

Varies.

29
Q

What ion has the same electron configuration as argon?

A

Chloride ion.

30
Q

Do metals tend to gain or lose electrons?

A

Lose

31
Q

Do nonmetals tend to gain or lose electrons?

A

Gain.

32
Q

Noble gases are ____ in chemical reactions

A

nonreactive

33
Q

Anions and cations attract each other by means of ____.

A

electrostatic forces.

34
Q

The forces of attraction that hold ions together..

A

Ionic bonding.

35
Q

What are the charge of ions?

A

neutral.

36
Q

Why do ions have a neutral charge?

A

The positive charge of cations equals the negative charge of anions.

37
Q

What is the lowest whole number ration of ions?

A

Formula unit.

38
Q

Almost all ionic compounds are in what state of matter in room temp?

A

Solid.

39
Q

Ionic compounds have what type of structure?

A

Very organized, crystal.

40
Q

When do ionic compounds conduct an electric current?

A

When in the liquid state or dissolved in water.

41
Q

The number of ions of opposite charge surrounding each ion in a crystal?

A

Coordination number.

42
Q

Do ionic bonds have high or low melting points?

A

High.

43
Q

Why is an ionic compounds able to conduct electric current when melted/is a liquid?

A

The orderly structure breaks down & cations are able to move freely. It allows electric current to flow between the electrodes.

44
Q

Most group 1A cations have how many valence electrons?

A

One to three.

45
Q

Metals consist of what?

A

Closely packed cations that are surrounded by a sea of cations.

46
Q

Why are metals malleable and ductile?

A

Particles are able to slide past each other.

47
Q

What are the three ways in which metals can be arranged?

A

Body-centered, face-centered, and close-packed.

48
Q

The attraction of valence electrons for positive metal ions?

A

Metallic bonds.

49
Q

What is a mixture of two or more elements, at least one of which is a metal?

A

Alloy.

50
Q

What type of alloy whose component atoms are different sizes (smaller ones fit into the spaces of the larger ones)?

A

Interstitial alloy.

51
Q

Why are metals good conductors of heat?

A

Electrons can flow freely.

52
Q

Alloys that are the same size?

A

Substitutional alloy.

53
Q

How many neighbors does a body-centered cubic structure have (except those on the surface)?

A

Eight

54
Q

How many neighbors does a face-centered cubic arrangement have?

A

Twelve.

Chemistry (12 decks)

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