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Chem 12U > Chemical Bonding Chapter 4 > Flashcards

Chemical Bonding Chapter 4 Flashcards

1
Q

What does VSEPR stand for

A

Valence Shell Electron Pair Repulsion Theory

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2
Q

A region of space in which there is a high probability of finding an electron

A

Orbital

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3
Q

What is the shape of the p orbital?

A

Dumbbell

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4
Q

What is the shape of the s orbital?

A

Sphere

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5
Q

What is the shape of the d orbital

A

“Four-leaf Clover”

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6
Q

What is the most electronegative element

A

Fluorine

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7
Q

What is the least electronegative element

A

Francium

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8
Q

-They are three-dimensional

-They can contain a maximum of two electrons

-Their shapes are predicted by Schrodinger’s equation

A

Orbital

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9
Q

Substances that are non-conductors and soluble in water
(if not too large)

A

Molecular Crystals

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10
Q

A substance is a solid that is ductile and malleable and conducts electricity and heat in the solid state.

A

Metal

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11
Q

Dissolves in water and conducts electricity when dissolved or in the molten state

A

Ionic Substance

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12
Q

According to VSEPR theory, molecules adjust their shapes to keep what as far apart as possible?

A

Pairs of valence electron orbitals

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13
Q

A partial positive charge at one end of a molecule combined with a partial negative charge at the other end of a molecule

A

Dipole

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14
Q

What causes high surface tension in water?

A

Hydrogen Bonding

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15
Q

Must have this in order to form double and triple bonds

A

p-orbital

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16
Q

Bond type in double and triple bonds only

A

pi-bond

17
Q

Uneven sharing of electrons

A

Polar Bond

18
Q

A combination of at least two different orbitals

A

Hybrid Orbital

19
Q

3-D arrangement of covalent bonds between atoms

A

Covalent Network

20
Q

Weak forces between all molecules

A

London Dispersion Forces

21
Q

Attraction associated with the transfer of electrons

A

Ionic Bond

22
Q

Attraction between polar molecules

A

Dipole-Dipole Force

23
Q

Any force occurring between molecules

A

Intermolecular Forces

24
Q

Forces that hold atoms together

A

Intramolecular Forces

24
Q

A regular repeating pattern of atoms, ions, or molecules

A

Crystal Lattice

25
Q

If the electronegativity difference is 0 to 0.4 inclusive

A

Nonpolar Covalent

26
Q

If the electronegativity difference is >0.4 to 1.7 inclusive

A

Polar Covalent

27
Q

if the electronegativity difference is >1.7 to 4.0 inclusive

A

Ionic

28
Q

How do you find the bond polarity?

A

Calculate the electronegativity difference between a bond of a molecule

29
Q

How do you find the polarity of a molecule?

A

Step 1: find the EN difference between each bond

Step 2: does the molecule have only non-polar bonds if so then the molecule is non-polar. If the molecule has polar bonds move to next step

Step 3: If the molecule is diatomic(1 bond)then the molecule is polar. If the molecule is polyatomic( more than 1 bond) then move on to step 4

Step 4: If the shape of the molecule is not symmetrical then the molecule is polar. If the shape of the molecule is symmetrical move to step 5

Step 5: if the molecules bonded to the central atom are not the same then the molecule is polar. If the molecules bonded to the central are the same the molecule is non-polar

30
Q

Ionic Crystals properties?

A

-positive metal and nonmetal ions

-primary force of attraction is ionic bonds through electrostatic forces

-High boiling and melting points

-Conducts electricity when liquid(molten) or dissolved in solution

-Does not conduct as a solid

-Hard Brittle Solid

-Transfer of electrons is necessary to be formed

Examples: NaCl MgO CaCO3

31
Q

Metallic Crystals properties?

A

-Closely packed metal atoms

-Mettalix bonding through electrostatic interactions of free moving electrons

-Boiling and melting point varies from low to high (mercury and tungsten)

  • Good conductor of both heat energy and electricity when solid

-Sheen: silver and shiny, Malleability & Hardness: Gold is soft and Al is hard

-the condition necessary to form is the “electron sea theory”

Examples: Au, Al, Cu

32
Q

What causes Metallic Crystals to have properties?

A

-Sheen: Mobile valence electrons absorb and emit light energy of many wavelengths of light

-Malleability: The “electron sea” allows atoms to slide over each other.

Electrical conductivity: Mobile valence electrons produce an electric current when a metal is connected to a battery

-Hardness: The “electron sea” surrounding the positive nuclei produces strong electrostatic attractions that hold the nuclei together.

33
Q

Molecular Crystal properties?

A

-molecules create the crystals

-Inter molecular forces such as h-bonding, dipole-dipole and LDF are the primary force of attraction

-Lower melting points than ionic crystals as IMF are weaker than ionic bonds

-Does not conduct well as solid or when dissolved in a solution

-Softer than ionic crystals

-composed of neutral molecules in order to form

Examples: Ice, Dry Ice, Iodine

34
Q

Covalent Network Crystal properties?

A

-Atoms are involved in creating this crystal

-Covalent bonds between the atoms is primary force of attraction

-High melting point because of the strong covalent bonds

  • Does not conduct electricity well as the electrons are unable to move freely. They are also insoluble so can’t dissolve in solutions
  • Extreme Hardness

-Has a interlocking network structure which allows it to form

-Examples: Diamond, C

35
Q

What does the polarity of a molecule define?

A

-surface tension
-melting and boiling point temperatures
-solubility in certain solvents.

36
Q

How do Polar molecules interact?

A

Polar molecules interact through intermolecular forces such as hydrogen bonding or dipole-dipole bonding.

Chem 12U (5 decks)

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