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Chem > Ch 6 Section 3 > Flashcards

Ch 6 Section 3 Flashcards

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1
Q

A familiar example of an ionically bonded compound is

A

Sodium chloride

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2
Q

A sodium atom, NA+ has a charge of

A

1+

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3
Q

A chloride ion, Cl- has a charge of

A

1-

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4
Q

There is an electrical force of attraction between

A

Oppositely charged ions

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5
Q

In sodium chloride the oppositely charged ions combine in a one to one ratio so that each positive charge is

A

Balanced by a negative charge

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6
Q

An ionic compound is composed of positive and negative ions that are

A

Combined so that the numbers of positive and negative charges are equal

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7
Q

Most ionic compounds exist as

A

Crystalline solids

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8
Q

A crystal of any ionic compound is a 3-dimensional network of

A

Positive and negative ions mutually attracted to one another

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9
Q

In contrast to a molecular compound an ionic compound is not composed of

A

Independent neutral units that can be isolated and examine s

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10
Q

The chemical formula of an ionic compound merely represents the

A

Simplest ratio is the compounds combined ions that gives electrical neutrality

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11
Q

The chemical formula of an ionic compound shows the ratio of the i

A

Ions present in a sample of any size

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12
Q

A formula unit is the simplest collection of atoms from which an

A

Ionic compounds formula can be established

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13
Q

In the naming of a monatomic anion the ending of the elements name is replaced with

A

-ide

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14
Q

Most of the rocks and minerals that make up earths crust consist of

A

Positive and negative ions held together by ionic bonding

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15
Q

The ratio of ions in a formula unit depends on the

A

Charles of the ions combined

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16
Q

Electron for notation can be used to demonstrate the

A

Changes that take place in ionic bonding

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17
Q

Ionic compounds do not ordinarily form by the

A

Combination of isolated atoms

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18
Q

Atoms it sodium and other alkali metals readily lose one electron to

A

Form cations

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19
Q

Atoms of chlorine and other halogens readily gain one electron to

A

Form anions

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20
Q

The combination of sodium and chlorine atoms to produce one formula unit of sodium chloride can be represented as follows

A

Sodium atom + chlorine atom –> sodium cation + chlorine anion

(Refer to txtbk for electron dot notation)

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21
Q

The transfer of an electron from the sodium atom to the chlorine atom transforms each atom into an ion with a

A

Noble gas configuration

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22
Q

In an ionic crystal ions minimize their potential energy by combining in an

A

Orderly arrangement known as a crystal lattice

23
Q

The attractive forces at work within an ionic crystal include those between

A

Oppositely charged and those between the nuclei and electrons of adjacent ions

24
Q

The repulsive forces at work within an ionic crystal include those between

A

Like-charged ions and those between electrons of adjacent ions

25
Q

The distances between ions and their arrangement in a crystal represent a

A

Balance among all these forced

26
Q

In NaCl attraction between the adjacent oppositely charged ions is much stronger than

A

Repulsion by other ions or the same charge which are farther away

27
Q

The 3-dimensional arrangements of ions and the strength of attraction between them vary with the

A

Sizes and charges of the hind and the numbers of ions of different charges

28
Q

To compare bond strengths in ionic compounds chemists compare the amounts of energy

A

Releases when separated ions in a gas come together to form a crystalline solid

29
Q

Lattice energy is the energy released when one

A

Nike of an ionic crystalline compound is formed from gaseous ions

30
Q

The negative lattice energy values indicate that energy is

A

Released when the crystals are formed

31
Q

The force that holds ions together in ionic compound is a very strong overall

A

Attraction. Between positive and negative charges

32
Q

The forces of attraction between molecules are much… Than the forces among formula…

A

Weaker than the forces among formula units in ionic bonding

33
Q

This difference in the strength of attraction between the basic units of molecular and ionic compounds gives rise to

A

Different properties in the two types or compounds

34
Q

The melting pt, boiling pt, and harness of a compound depend on how

A

Strongly it’s basic units are attracted to each other

35
Q

Because the forces of attraction between individual molecules are not very strong many molecular compounds melt at

A

Low temperatures

36
Q

Many molecular compounds are completely…. At room temperature

A

Gaseous

37
Q

The ions in ionic compounds are held together by strong attractive forced do ionic compounds generally have higher

A

Melting and boiling points than do molecular compounds

38
Q

Ionic compounds are hard but

A

Brittle

39
Q

In an ionic crystal even a slight shift of one town of ions relative to another causes a large

A

Buildup of repulsive forces

40
Q

These repulsive forces in the ionic crystals make it difficult for one layer to move

A

Relative to another, causing ionic compounds to be hard

41
Q

If one layer is moved, however, the repulsive forces make the layers part

A

Completely, causing ionic compounds to be brittle

42
Q

In the solid state, ions cannot move, so the compounds are not

A

Electrical conductors

43
Q

In the solid state, ions cannot move, so the compounds are not

A

Electrical conductors

44
Q

In the molten state, ionic compounds are electrical conductors because the ions can move

A

Freely to carry electrical current

45
Q

Many ionic compounds can…in water

A

Dissolve

46
Q

When ionic compounds dissolve their ions separate from each other and become

A

Surrounded by water molecules

47
Q

These ions are free to move through the solution so sucks solutions are

A

Electrical conductors

48
Q

Other ionic compounds do not dissolve in water, however, because the attractions between the water molecules and the ions cannot overcome the

A

Attraction. Between the ions

49
Q

Certain aims bond covalently with each other to form a group of atoms that has both

A

Molecular and ionic characteristics

50
Q

A poly atomic ion is a charged group of

A

Covalently bonded atoms

51
Q

Poly atomic ions combine with ions of opposite charge to form

A

Ionic compounds

52
Q

The charge of a poly atomic ion results from an excess of

A

Electrons (negative charge) or a shortage of electrons (positive charge)

53
Q

If the ion is negatively charged add to the total number of cal me electrons a number of electrons corresponding to the

A

Ions negative charge

54
Q

If the ion is positively charged, subtract from the total number of valence electrons s number of the electrons corresponding not to the ions

A

Positive charge

Chem (54 decks)

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