Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry > Types of Bonding > Flashcards

Types of Bonding Flashcards

(88 cards)

Start Studying
1
Q

What is metallic bonding?

A

Metallic bonding is the force of attraction between free-floating valence electrons and positively charged metal ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

True or False: Metallic bonds are formed between nonmetal atoms.

A

False

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What do we call the electrons that are free to move in metallic bonding?

A

Delocalized electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Fill in the blank: In metallic bonding, metal atoms lose their __________ to form positively charged ions.

A

Valence electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Which property of metals is primarily due to metallic bonding?

A

Electrical conductivity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is the term for the structure formed by metal atoms in a solid state?

A

Metallic lattice

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

True or False: Metallic bonds are typically stronger than ionic bonds.

A

False

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is one key characteristic of metals that arises from metallic bonding?

A

Malleability

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Multiple Choice: Which of the following is NOT a property of metals? A) Ductility B) High melting points C) Brittle D) Good conductivity

A

C) Brittle

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What happens to the electrons in a metal when it is subjected to stress?

A

The delocalized electrons can move, allowing the metal to deform without breaking.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is the role of delocalized electrons in metallic bonding?

A

They provide cohesion and contribute to the electrical conductivity of the metal.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Fill in the blank: The ability of metals to be drawn into wires is known as __________.

A

Ductility

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is the effect of temperature on metallic bonding?

A

Increased temperature can increase the movement of atoms and weaken the metallic bond.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

True or False: Metallic bonds can be found in both pure metals and alloys.

A

True

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What type of bond is present in alloys?

A

Metallic bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Multiple Choice: Which property is NOT associated with metallic bonding? A) Thermal conductivity B) Low boiling point C) High density D) Lustrous appearance

A

B) Low boiling point

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What is the primary reason metals are good conductors of electricity?

A

The presence of delocalized electrons that can move freely.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What structure do you typically find in metallic solids?

A

A closely packed arrangement of atoms.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Fill in the blank: The __________ model helps explain the properties of metallic bonding.

A

Sea of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What is the significance of the coordination number in metallic bonding?

A

It indicates the number of nearest neighbors surrounding a metal atom in a lattice.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

True or False: Metals have a fixed shape due to strong covalent bonds.

A

False

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What is the effect of alloying on the properties of metals?

A

Alloying can enhance strength, corrosion resistance, and other physical properties.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Fill in the blank: The __________ structure of metals allows them to conduct heat efficiently.

A

Crystalline

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What is the relationship between the number of delocalized electrons and the strength of metallic bonding?

A

More delocalized electrons typically result in stronger metallic bonds.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Multiple Choice: Which of the following metals has the highest melting point? A) Sodium B) Iron C) Mercury D) Lead
B) Iron
26
What occurs to the metallic bond when a metal is heated?
The bond weakens as the kinetic energy of the atoms increases.
27
True or False: Metallic bonds are directional.
False
28
What is one reason metals are malleable?
The layers of atoms can slide over each other without breaking the metallic bond.
29
Fill in the blank: The __________ effect is the reason metals appear shiny.
Photoelectric
30
What is the typical bond strength of metallic bonds compared to covalent bonds?
Metallic bonds are generally weaker than covalent bonds.
31
True or False: All metals have the same metallic bonding characteristics.
False
32
What happens to the conductivity of metals as temperature increases?
Conductivity decreases due to increased scattering of electrons.
33
What is an example of a property that shows the ductility of metals?
The ability to be stretched into wires.
34
Multiple Choice: Which of the following is a common use for metals due to their properties? A) Insulation B) Construction C) Fuel D) Water purification
B) Construction
35
What is the role of metallic bonding in the strength of materials?
Metallic bonding contributes to the overall strength and stability of metallic structures.
36
What is ionic bonding?
Ionic bonding is the electrostatic attraction between oppositely charged ions.
37
True or False: Ionic bonds are formed between two nonmetals.
False
38
Fill in the blank: Ionic compounds are generally formed between _____ and nonmetals.
metals
39
What charge do cations carry?
Cations carry a positive charge.
40
What charge do anions carry?
Anions carry a negative charge.
41
Give an example of an ionic compound.
Sodium chloride (NaCl).
42
What is the typical structure of ionic compounds?
Ionic compounds typically form a crystalline lattice structure.
43
Multiple choice: Which of the following is a property of ionic compounds? A) High melting point B) Low solubility C) Poor electrical conductivity D) All of the above
A) High melting point
44
What happens to ionic compounds when they dissolve in water?
They dissociate into their constituent ions.
45
True or False: Ionic compounds conduct electricity in solid form.
False
46
What is lattice energy?
Lattice energy is the energy released when gaseous ions combine to form an ionic solid.
47
Multiple choice: Which factor increases lattice energy? A) Larger ion size B) Greater charge of ions C) Increased distance between ions D) None of the above
B) Greater charge of ions
48
What is the role of electronegativity in ionic bonding?
Electronegativity differences between atoms determine the formation of ionic bonds.
49
Fill in the blank: The greater the difference in electronegativity between two atoms, the _____ the ionic character of the bond.
greater
50
What is the typical physical state of ionic compounds at room temperature?
Ionic compounds are typically solid at room temperature.
51
True or False: Ionic compounds are usually soluble in polar solvents.
True
52
What is a common test for the presence of ionic compounds?
Testing for electrical conductivity in solution.
53
What type of ions do alkali metals form?
Alkali metals form cations.
54
What type of ions do halogens typically form?
Halogens typically form anions.
55
Multiple choice: Which of the following describes ionic bonds? A) Weak B) Strong C) Very weak D) None of the above
B) Strong
56
What determines the solubility of an ionic compound in water?
The balance between lattice energy and hydration energy.
57
Fill in the blank: Ionic compounds tend to have _____ melting and boiling points.
high
58
What happens to the ions in an ionic compound when it is melted?
The ions become free to move and can conduct electricity.
59
True or False: Ionic bonds can be broken by heat.
True
60
What is the primary reason for the high melting points of ionic compounds?
The strong electrostatic forces between the ions.
61
What type of crystal structure do ionic compounds exhibit?
They exhibit a face-centered cubic or hexagonal close-packed structure.
62
What is the effect of ionic bonding on the physical properties of compounds?
Ionic bonding results in high melting points, solubility in water, and electrical conductivity in solution.
63
What type of bond is formed by the sharing of electron pairs between atoms?
Covalent bond
64
True or False: Covalent molecular compounds typically have high melting and boiling points.
False
65
Fill in the blank: Covalent network bonding involves a continuous network of __________ between atoms.
covalent bonds
66
What is a characteristic property of covalent molecular compounds?
They are usually gases or liquids at room temperature.
67
Which of the following is an example of a covalent network solid? (A) Water (B) Diamond (C) Sodium chloride
B) Diamond
68
True or False: Covalent network solids are typically poor conductors of electricity.
True
69
What type of structure do covalent molecular compounds form?
Discrete molecules
70
In covalent network bonding, atoms are bonded in a __________ arrangement.
three-dimensional
71
Which of the following properties is NOT associated with covalent molecular compounds? (A) Volatility (B) High thermal conductivity (C) Low solubility in water
B) High thermal conductivity
72
What is the primary force holding covalent molecular compounds together?
Intermolecular forces
73
True or False: Covalent network solids have defined melting points.
False
74
What type of atoms typically form covalent bonds?
Nonmetals
75
What is the general state of covalent molecular compounds at room temperature?
Gas or liquid
76
Fill in the blank: In covalent network solids, the atoms are bonded by __________ bonds throughout the entire structure.
covalent
77
What is an example of a covalent molecular compound?
Methane (CH4)
78
True or False: Covalent network solids tend to be brittle.
True
79
What is the common property of covalent network solids regarding hardness?
They are usually very hard.
80
Which type of bonding is characterized by localized electron sharing?
Covalent molecular bonding
81
What is the effect of covalent bonding on the solubility of compounds in water?
Many covalent molecular compounds are insoluble in water.
82
Fill in the blank: Covalent network solids have __________ melting and boiling points compared to covalent molecular compounds.
higher
83
True or False: Covalent molecular compounds can conduct electricity in solid form.
False
84
What is the term for the energy required to break a covalent bond?
Bond dissociation energy
85
Which of the following is a property of covalent network solids? (A) Low density (B) High thermal stability (C) Good electrical conductivity
B) High thermal stability
86
What determines the shape of a covalent molecular compound?
The arrangement of electron pairs around the central atom.
87
Which type of covalent bond involves the equal sharing of electrons?
Nonpolar covalent bond
88
What is the result of covalent bonding on the overall charge of the molecule?
The molecule remains neutral.

Chemistry (6 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions