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Grade 8 science > Chemical bonding > Flashcards

Chemical bonding Flashcards

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1
Q

What is an atomic number? [1]

A

An atomic number is a number that gives a number of protons.

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2
Q

What is a mass number? [1]

A

neutron + proton= mass number

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3
Q

How much do proton, neutron, and electron way? [2]
What is the charge of proton, neutron, and electron? [2]

A

proton, neutron 1
electron 1/2000
proton is charged as positive
neutron is not charged
electron is chared as negative

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4
Q

What is an electron shell and what is the maximum number of electrons in one shell? [2]

A

The outside part of an atom around the atomic nucleus. And the maximum number of the electron shell is 8.

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5
Q

What is the trend of boiling point and melting point in group 1? [1]

A

As you go down, melting point and the boiling point decrease in group 1

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6
Q

What are the trend of the melting point and the boiling point in group 7? [1]

A

As you go down, the boiling point and the melting point increase in group 7.

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7
Q

What are the trends of boiling point and melting point in group 0? [1]

A

As you go down, the melting point and the boiling point increase in group 0.

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8
Q

Explain the trend of reactivity in group one. [1]

A

As you go down in group 1, the reactivity increase.

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9
Q

Write a word equation and the symbolic equation for the reaction with group 1 element and water. [2]

A

Lithium+water=hydrogen+lithium hydroxide
Li+H20=H2+LiOH

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10
Q

What is a ionic bonding?[1]

A

A link formed between two or more ions to form a compound.

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11
Q

What is covalent bonding?[1]

A

A link formed when atoms share electrons to form a molecule.

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12
Q

Explain why ionic compounds have a high melting point and high boiling. [1]

A

Ionic compound is held together by strong electrostatic forces that require high energy to break.

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13
Q

Write the formula of fluorine ion and fluorine compound.[2]

A

F-, F

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14
Q

What is a lattice structure?

A

A regular repeated three-dimensional arrangement of atoms ions or molecules in a metal or other crystalline solid.

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15
Q

Suggest why sulfur conducts electricity as a liquid but does not conduct electricity as a solid. [3]

A

Sulfur can’t conduct electricity when it’s solid because electrons are not delocalized. But when sulfur turns to liquid it can conduct electricity because electrons are delocalized

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16
Q

Describe the structure and bonding in sodium chloride.[4]

A

I think Sodium chloride is a giant ionic structure. Na+ Cl-. electrostatic forces of attraction hold the ion together.
Ionic bonding.

17
Q

Explain why iodine has a low melting point. [3]

A

Iodine is held by weak intermolecular forces and requires a low melting point. small/simple covalent.

18
Q

in terms of particles why liquid iodine does not conduct electricity[1]

A

no delocalised electron and mobile charge carrrier

19
Q

Explain the boiling and melting point of giant ionic bonding[3]

A

Ionic bonding has high melting and boiling pt because strong electrostatic forces of attraction held them together which requires high energy to break.

20
Q

Explain the boiling and melting pt of simple covalent[3]

A

Simple covalent has weak intermolecular force between molecules so it requires little energy to break.

21
Q

Explain the boiling and melting pt of giant Metallic[3]

A

Giant metallic has high melting pt and boiling pt because electrostatic forces of attraction hold them (between positive metal ions and delocalised electrons) together which requires high energy to break.

22
Q

Explain the boiling and melting pt of giant covalent [3]

A

Giant covalent have high melting pt and boiling pt because they have strong covalent bonding holding them together which requires high energy to break.

23
Q

Does Ionic bonding compound conduct electricity? [3]

A

Doesn’t conduct because delocalized electrons are not free to move but when it’s molten or aqueous because delocalized electrons can move freely and it can carry charges through the structure.

24
Q

Does Ionic bonding compound conduct electricity? [3]

A

Doesn’t conduct because delocalized electrons are not free to move but when it’s molten or aqueous because delocalized electrons can move freely and it can carry charges through the structure.

25
Q

Can giant Ionic bonding compound conduct electricity? [3]

A

Doesn’t conduct because delocalized electrons are not free to move but when it’s molten or aqueous(dissolved) it can because delocalized electrons can move freely and it can carry charge particles through the structure.

26
Q

Can simple covalent conduct electricity?

A

No, because there are no charged particles to carry charges through the structure.

27
Q

Can giant covalent conduct electricity?

A

No because there are no delocalized electrons because strong covalent bonding hold them but graphite can because it only has a strong covalent bond between molecules but between layers, there is a weak intermolecular force holding them so electrons is delocalised.

28
Q

Can giant metallic compound conduct electricity?[3]

A

Yes it can because electrons are delocalised so it can carry charged particles through the structure.

29
Q

Explain the structure and bonding of giant ionic compounds.

A

Ionic has a lattice( an ordered set of points that define the structure of a crystal-forming particle.) structure and it is held by the electricstatic force of attraction between positive and negative ions

30
Q

Explain the structure and bonding of , simple covalent compound

A

Simple covalent has a structure of small molecules and particles are bonded together by strong covalent bonds but molecules are bonded together by weak intermolecular forces.

31
Q

Explain the structure and bonding of giant covalent compound.

A

Giant covalent has giant lattice sturcture and it is bonded together by strong covalent bonding.

31
Q

Explain the structure of metallic compound

A

Positive metal ions in a sea of delocalized electrons. Held together by electrostatic force of attraction between positive ions and electrons.

Grade 8 science (2 decks)

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