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Chemistry Yr 11 > Chemical Bonding (Intramolecular) > Flashcards

Chemical Bonding (Intramolecular) Flashcards

1
Q

Ionic Bonding is between ____________ &____________________

A

Ionic Bonding is between METALS & NON-METALS

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2
Q

In an Ionic Bond Metals ________electrons, giving it a __________ charge

A

In an Ionic Bond Metals LOSE electrons, giving it a POSITIVE charge

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3
Q

In an Ionic Bond Non- Metals ________electrons, giving it a __________ charge

A

In an Ionic Bond Non- Metals GAIN electrons, giving it a NEGATIVE charge

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4
Q

What is a Cation?

A

Positive Ion

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5
Q

What is a Anion?

A

Negative Ion

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6
Q

What is the Ionic Lattice?

A

Positive and negative ions attract each other to form a three dimensional continuous lattice structure.

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7
Q

The _______ is written first in the ionic formula

A

Cation (Metal)

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8
Q

Ionic Bonding- Boiling Point

A

High. The is a large amount of thermal energy required to separate the ions which are bound by strong electrostatic forces.

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9
Q

Ionic Bonding- Electro conductivity in Solid

A

No- there are no mobile charge particles to conduct an electric current

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10
Q

Ionic Bonding- Electro conductivity in Liquid

A

Yes- the cations and anions are able to move and conduct electricity

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11
Q

Ionic Bonding- Hardness

A

Very Hard- The surface of crystals are not easily scratched as the ions are strongly bound and not easily displaced

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12
Q

Ionic Bonding- Brittleness

A

Very Brittle- Shatter if you try to distort is. Distortion causes ions of like charges to come together and repel sharply

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13
Q

Covalent Bonding is between ________

A

Covalent Bonding is between NON-METALS

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14
Q

Covalent Bonding is the __________ of electrons

A

Covalent Bonding is the SHARING of electrons

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15
Q

Ionic Bonding is the ____________ of electrons

A

Ionic Bonding is the TRANSFER of electrons

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16
Q

In covalent Bonding electrons are shared according to ______________

A

In covalent Bonding electrons are shared according to ELECTRONEGATIVITY

17
Q

Covalent Bonding- Electroconductivity

A

No- there are no mobile charged particles as the electrons are bound tightly to the atoms or are shared by atoms in covalent bonds

18
Q

Covalent Bonding- Melting and Boiling Points

A

Low- the forces of attraction between molecules are weak, requiring a small amount of thermal energy to seperate

19
Q

Covalent Bonding- Hardness

A

Soft- The molecules are weakly attracted to each other and are easily displaced

20
Q

What is Covalent Network?

A

Do not form separate discrete molecules but a continuous network

21
Q

Covalent Network- Electrical Conductivity

A

Poor- electrons are held tightly together on atoms or within covalent bonds, preventing electrons from moving through the lattice. Graphite is the exception as it has a free electron

22
Q

Covalent Network- Melting Point

A

Very High- the atoms are bound by strong covalent bonds. In order to break the many covalent bonds a large amount of thermal energy is required

23
Q

Covalent Network- Hardness

A

Strong- the atoms are strongly bound and not easily displaced

24
Q

Covalent Network- Brittleness

A

Very Brittle- when a sufficient amount of force is applied to break the covalent bond, the lattice is distorted.

Covalent Networks shatter rather than deform

25
Q

What is Metallic Bonding?

A

A Metallic Bonds are the delocalised electrons moving over tightly packed metal cations

26
Q

Metals- Density

A

Very Dense- the particles present in Metals are tightly packed in a lattice

27
Q

Metals- Melting & Boiling Points

A

High- a large amount of thermal energy is required to overcome the strong electrostatic attraction between the positive ions and delocalised electrons

28
Q

Metals- Heat and Electricity Conductors

A

Very Good- the delocalised electrons transmit the energy through vibrations from one positive ions to its neighbour

29
Q

Difference between Metals and Covalent Network

A

Metals have conduct electricity well, whereas Covalent Networks do not.

30
Q

Explain the difference in the Melting Points of different Metals.

E.g Potassium +1 is 64 degrees whereas Calcium Ca+2 is 850 degrees.

A

Metallic Ca+2 has twice as many delocalised electrons which create an electrostatic attraction that is twice as strong between the electrons and positive ions.

Chemistry Yr 11 (12 decks)

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