Chapter 4 - Chemical bonding Flashcards

1
Q

What is dative/coordinate bonding?

A

When the two shared electrons come from the same atom

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2
Q

What angle and shape does a molecule with two bond pairs make?

A

180 degrees, and linear

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3
Q

What angle and shape does a molecule with three bond pairs make?

A

120 degrees, and trigonal planar

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4
Q

What angle and shape does a molecule with four bond pairs make?

A

109.5 degrees, and tetrahedral

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5
Q

What angle and shape does a molecule with five bond pairs make?

A

120 and 90 degrees, and trigonal bipyramid

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6
Q

What angle and shape does a molecule with six bond pairs make?

A

90 degrees, octahedral

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7
Q

What angle and shape does a molecule with three bond pairs and 1 lone pair make?

A

107 degrees, and pyramidal

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8
Q

What angle and shape does a molecule with two bond pairs and 2 lone pairs make?

A

104.5 degrees, and bent/angular

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9
Q

What is an examples of bent molecules?

A

water

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10
Q

What angle and shape does a molecule with four bond and 2 lone pairs make?

A

90 degrees, and square planar

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11
Q

What is the formula of ammonia

A

NH3

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12
Q

What is the formula of ammonium

A

NH4

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13
Q

What are the three main types of intermolecular forces?

A

Hydrogen bonds, Van der Waals, permanent dipole-dipole forces

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14
Q

What is another name for ionic bonds?

A

Electrovalent bonds

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15
Q

What do bond lengths depend on?

A

How strong the force of attraction is, which results in a stronger bond

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16
Q

What do the shape of bond angles depend on?

A

The numbers of electron pairs and bond pairs surrounding each atom

17
Q

Which bond occurs when hybridized orbitals overlap linearly?

A

Sigma bonds

18
Q

Which bond occurs when hybridized orbitals overlap sideways ?

A

pi bonds

19
Q

Describe the attraction forces between metallic bonding

A

a regular lattice structure made up of strong electrostatic forces between positive charges and the negative charges of delocalised electrons

20
Q

What are the factors that increase the strength of metallic bonding

A

increasing positive charge on the ions, decreasing the size of metal ions, increasing numbers of mobile electrons per atom

21
Q

Which are more reactive, dipoles or non-polar molecules?

A

Dipoles

22
Q

Why can graphite conduct electricity, and graphite cannot?

A

Graphite has delocalised electrons, while diamond does not

23
Q

What causes the increase of Van der Waals’?

A

Increased number of electrons (and the protons),

Increasing the number of contact points between molecules (work best will crystalline structures)

24
Q

Which elements are needed to be present for hydrogen bonding to occur?

A

Fluorine, oxygen or nitrogen, that have an available lone pair

25
Q

What properties did hydrogen bonding give water?

A

High enthalpy change of evaporation and boiling point, surface tension and viscosity, ice is less dense than water (because of the three-dimensional hydrogen bonded network of water molecules)

26
Q

What are some properties of covalent bonds in room temperature?

A

they are usually liquid or gas, they have low melting points, low boiling points, and low enthalpy changes of vaporisation. If they are solid in room temperature that means that their Van der Waal forces are very high

27
Q

What interaction occurs when ionic bonds dissolve in water?

A

ion-dipole interactions