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Bonding Flashcards

1
Q

What are the two types of covalent substances?

A

Covalent network substances and covalent molecular substances

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2
Q

What is an example of a covalent network substance?

A

Diamond

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3
Q

What are the melting points and hardness of covalent network substances?

A

Very high melting points and very hard

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4
Q

What type of bonds hold carbon atoms together in diamond?

A

Strong covalent bonds

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5
Q

What are the melting and boiling points of covalent molecules like oxygen and water?

A

Low melting points and boiling points

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6
Q

What states can covalent molecules exist in at room temperature?

A

Liquid, gas, or low melting point solid

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7
Q

Do covalent compounds conduct electricity?

A

No, except for water

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8
Q

What bonds are broken when ice is melted?

A

Weak bonds between the molecules

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9
Q

True or False: Graphite is a covalent network that conducts electricity.

A

True

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10
Q

Why does graphite conduct electricity?

A

It has delocalised (free to move) electrons

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11
Q

What type of substance is titanium tetrachloride (TiCl4)?

A

Covalent molecular substance

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12
Q

What are the melting and boiling points of titanium tetrachloride?

A

Low melting and boiling points

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13
Q

Fill in the blank: Covalent network substances have very high _______.

A

Melting points

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14
Q

Fill in the blank: _______ is an exception to the rule that covalent compounds do not conduct electricity.

A

Water

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15
Q
A
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16
Q
A
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17
Q

What determines the properties of a substance?

A

The types of bonds that hold its atoms together

Different types of bonds influence physical and chemical properties.

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18
Q

What structure do ionic compounds form?

A

Lattice structure

This is a regular arrangement of metal and non-metal ions.

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19
Q

What is a characteristic shape of ionic compounds when observed closely?

A

Cube-like structure

A simple grain of salt exemplifies this structure.

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20
Q

What is a key property of ionic compounds regarding melting points?

A

High melting point

Millions of strong ionic bonds must be broken to melt an ionic compound.

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21
Q

How do ionic compounds behave when molten or in solution?

A

They conduct electricity

Ionic compounds conduct electricity when ions are free to move.

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22
Q

Do ionic compounds conduct electricity when solid?

A

No

Ionic compounds do not conduct electricity in solid form.

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23
Q

What happens to ionic compounds when they dissolve in water?

A

Their lattice breaks up completely to form free ions

This allows the solution to conduct electricity.

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24
Q

What is required to melt an ionic compound?

A

Lots of energy

This is due to the necessity of breaking strong ionic bonds.

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25
Are all ionic compounds cube-shaped?
No ## Footnote Various shapes can be created from ionic crystals.
26
What determines the properties of a substance?
The types of bonds that hold its atoms together ## Footnote Different types of bonds influence physical and chemical properties.
27
What structure do ionic compounds form?
Lattice structure ## Footnote This is a regular arrangement of metal and non-metal ions.
28
What is a characteristic shape of ionic compounds when observed closely?
Cube-like structure ## Footnote A simple grain of salt exemplifies this structure.
29
What is a key property of ionic compounds regarding melting points?
High melting point ## Footnote Millions of strong ionic bonds must be broken to melt an ionic compound.
30
How do ionic compounds behave when molten or in solution?
They conduct electricity ## Footnote Ionic compounds conduct electricity when ions are free to move.
31
Do ionic compounds conduct electricity when solid?
No ## Footnote Ionic compounds do not conduct electricity in solid form.
32
What happens to ionic compounds when they dissolve in water?
Their lattice breaks up completely to form free ions ## Footnote This allows the solution to conduct electricity.
33
What is required to melt an ionic compound?
Lots of energy ## Footnote This is due to the necessity of breaking strong ionic bonds.
34
Are all ionic compounds cube-shaped?
No ## Footnote Various shapes can be created from ionic crystals.
35
What is a molecule?
A molecule is two or more atoms joined together by covalent bonds.
36
What types of atoms usually make up a molecule?
Molecules are usually made up of non-metal atoms only.
37
Give an example of a molecule.
Water (H₂O) is an example of a molecule.
38
What is a covalent bond?
A covalent bond is a shared pair of electrons between two non-metal atoms.
39
How do atoms become stable like noble gases?
Atoms become stable by having a full outer energy level.
40
How many outer electrons does neon have?
Neon has eight outer electrons.
41
How many outer electrons does oxygen have?
Oxygen has six outer electrons.
42
How many electrons must oxygen gain to become stable?
Oxygen must gain two electrons to become stable.
43
How many outer electrons does hydrogen have?
Hydrogen has one outer electron.
44
How many electrons must hydrogen gain to achieve stability?
Hydrogen must gain one more electron to achieve stability.
45
What holds atoms together in a covalent bond?
The electrostatic force of attraction between the positive nuclei and the negatively charged electrons.
46
Fill in the blank: A molecule is made up of _______ or more atoms.
two
47
True or False: A molecule can consist of metal atoms.
False
48
What is the role of the electron in a covalent bond?
Electrons are shared between two non-metal atoms.
49
What does the saying 'opposites attract' describe in the context of covalent bonds?
The attraction between the positively charged nucleus and negatively charged electrons.
50
What effect is created by both nuclei trying to pull electrons toward themselves in a covalent bond?
'Tug-of-war' effect.
51
What is the electron arrangement of hydrogen?
One.
52
What happens when two hydrogen atoms share electrons?
They both have two outer electrons.
53
What noble gas do two hydrogen atoms achieve the same electron arrangement as?
Helium.
54
What is a diatomic element?
An element that exists as pairs of atoms rather than single atoms.
55
Name a diatomic molecule.
Oxygen (O2).
56
How many diatomic elements are there to learn?
Seven.
57
List the seven diatomic elements.
* Hydrogen (H2) * Nitrogen (N2) * Oxygen (O2) * Fluorine (F2) * Chlorine (Cl2) * Bromine (Br2) * Iodine (I2)
58
Complete the mnemonic for remembering diatomic elements: 'Faney Clany Owes Him Nothing _______ But _______.'
Ice; Fluorine.
59
What is essential to draw for all diatomic elements?
A diagram of the molecule showing all of the outer electrons.
60
What analogy helps to describe how a covalent bond holds atoms together?
'Tug-of-war' description.

Chemistry (6 decks)

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