Chemistry - Chemical Bonding Flashcards

1
Q

How do unstable atoms become stable?

A
  • Lose or gain electrons (forming cations or anions)

- Sharing valence electrons

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2
Q

What is Ionic Bonding?

A

Chemical bonding that occurs between metals and non-metal atoms. The metal atom lose electrons and forms a cation and the non-metal gains electrons, forming anions

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3
Q

Why do Ionic solids have a high melting and boiling point?

A

The ions are strongly attracted to one another and it requires a lot of energy to separate the ions.

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4
Q

Why are ionic solids brittle?

A

Because

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5
Q

Why do ionic solids not conduct electricity?

A

Strong attraction between the ions means that they will not move, thus unable to conduct an electrical current.

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6
Q

Do molten ionic substances and ionic solutions (dissolved in water) conduct electricity?

A

Yes, because the ions are free to move

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7
Q

Anions

A

Negatively charged, since they gained electrons

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8
Q

Cations

A

Positively charged, since they lost electrons

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9
Q

Covalent Bonding

A

Atoms fill up their outermost energy level by sharing electrons.

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10
Q

What does a covalent bond result in?

A

A molecule

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11
Q

Diatomic Molecules

A

Hydrogen (H2), Nitrogen (N2), Oxygen (O2), Flourine (Fl2) & Chlorine (Cl2)

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12
Q

Why do the valence electrons of a metallic bond become delocalised?

A

The atoms are very tightly packed, thus the valence electrons don’t spin around any particular atom and are free to move.

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13
Q

What does the metallic lattice consist of?

A

Positive metal cations surrounded by negative delocalised electrons

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14
Q

Are metallic lattices malleable or ductile?

A

Yes, they are bent and stretched to form long wire.

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15
Q

Doo metallic lattices conduct electricity well?

A

Yes, they always do.

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16
Q

What is the reason that a metallic lattice can always conduct electricity?

A

The delocalised electrons are free to move.

17
Q

Do the orbitals of a metallic bond overlap?

A

Yes

18
Q

Are valence electrons tightly packed?

A

No

19
Q

Octet Rule

A

All elements want 8 electrons in their last energy level in order to become stable (besides the first 5)

20
Q

Valence Electrons

A

Electrons Present in the last energy level

21
Q

Valency

A

The number of electrons an element is willing to lose, gain or share in order to become stable

22
Q

Noble Gases

A

Chemically stable