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Chem 150 > Module 4: Exam 3 > Flashcards

Module 4: Exam 3 Flashcards

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1
Q

Number of atoms in the unit cell of a simple cubic cell

A

1

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2
Q

Number of atoms in the unit cell of a body centered cubic

A

2

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3
Q

Number of atoms in the unit cell of a face centered cubic

A

4

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4
Q

What fraction of a cell is on the corner of a unit cell?

A

1/8

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5
Q

What fraction of a cell is on the edge of a unit cell?

A

1/4

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6
Q

What fraction of a cell is on the side of a unit cell?

A

1/2

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7
Q

Packing efficency of simple cubic

A

52%

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8
Q

Packing efficiency of body centered cubic

A

68%

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9
Q

Packing efficiency of face centered cubic

A

74%

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10
Q

What is a coordination number?

A

The number of other atoms that are touching a particular atom

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11
Q

Coordination number of simple cubic

A

6

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12
Q

Coordination number of body centered cubic

A

8

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13
Q

Coordination number of face centered cubic

A

12

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14
Q

Edge length formula of simple cubic

A

2r

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15
Q

Edge length formula of face centered cubic

A

2(sqrt 2) * r

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16
Q

Edge length formula of body centered cubic

A

4/(sqrt3) *r

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17
Q

Which cubic model has the least amount of space between the atoms?

A

Face centered cubic

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18
Q

Crystalline solids

A

rigidly held in place

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19
Q

Amorphous solids

A

free to move around

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20
Q

What type of electrons do metals have?

A

Electrons that are free to move around

This makes them good conductors of electricity since they can transfer kinetic energy

21
Q

Why are two neutral hydrogen atoms attracted to eachother?

A

As force of attraction increases, the potential energy decreases

This allows them to move to a state of lower potential energy

22
Q

What happens to two atoms when they get too close together?

A

There is repulsion between the two nuclei and there is electron-electron repulsion

23
Q

On a potential energy curve for the interaction of two atoms, where is change in potential energy 0?

A

At the bottom of the “sweet spot” dip

24
Q

On a potential energy curve for the interaction of two atoms, where do repulsive forces overcome the attractive forces?

A

Once potential energy crosses the x-axis and becomes positive

25
Q

As force of attraction increases, what happens to potential energy?

A

It decreases

Until a certain point where force of repulsion overcomes because two atoms are too close

26
Q

Bond length

A

the distance(r) that makes change in potential energy 0

27
Q

Would a deeper potential energy well result in a stronger or weaker bond?

A

Stronger

less potential energy (deeper) = greater force of attraction

28
Q

Why does an ionic solid have to be expressed by an empirical formula?

A

Because it can go on forever

Therefore, need to simplify to ratio because there is no exact amount

29
Q

Difference between ionic bond and covalent bond

A

Ionic bond involves the complete transfer of an electron (metal and nonmetal)

Covalent bond involves the sharing of electrons

30
Q

Percent ionic character

A

how ionic a bond is

31
Q

Why is bonding a continuum?

A

different differences in electronegativies make some bonds and charges stronger than others?

32
Q

What does electronegativity tell us?

A

In a polar covalent bond, it will tell us which atom the electron is going to be pulled towards

33
Q

Example of a pure nonpolar covalent

A

O2

there is no difference in electronegativities

34
Q

Example of an ionic bond

A

NaCl

large difference in electronegativies, complete transfer of electrons

35
Q

Which type of bond is normally the strongest?

A

Ionic

36
Q

How do you determine the most polar covalent?

A

The greatest difference in electronegativity

37
Q

How do you determine the most polar covalent?

A

The greatest difference in electronegativity

38
Q

Percent ionic character of a complete ionic bond

A

100%

39
Q

Percent ionic character of a complete covalent bond

A

0%

40
Q

Percent ionic character of Na-Cl

A

79%

nothing is perfect

41
Q

Percent ionic character of Na-Cl

A

79%

nothing is perfect

42
Q

Is polar or nonpolar covalent a stronger bond?

A

In general, nonpolar covalent is stronger

However, have to take into consideration things like electron-electron repulsion

43
Q

Why is bond length of Cl2 longer than H2?

A

Cl2 has a larger radius, which makes the length longer

also decreases the force of attraction, making the bond between H2 stronger

44
Q

When does the atomic radius argument for bond length NOT work?

A

Size argument is negligible within the same period

45
Q

Relationship between formal charges and force of attraction

A

Formal charges increase the force of attraction and strengthen the bond

46
Q

Relationship between lone pairs and force of attraction

A

Lone pairs weaken the force of attraction and weaken the strength of the bond

it also makes the bond longer, since it is weaker

47
Q

What can effect the length of a bond?

A

If the atoms have the same charge, this increases repulsion and resultingly lowers force of attraction, making a longer bond

48
Q

Is there a greater difference in electronegativity between row or column?

A

If you move up a column and 2 over, that is normally a greater difference than moving DIRECTLY up a column

49
Q

Coordination number of ions that are wedged between face centered? Only on edges?

A

6

Chem 150 (10 decks)

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