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Chemistry Honors > Bonding Unit > Flashcards

Bonding Unit Flashcards

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1
Q

What is a non-polar bond?

A

The electronegativity of the atoms is the same, and therefore the electron pair is shared equally, a bond of two atoms of the same element.

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2
Q

What is a polar bond?

A

The electronegativities of the atoms are different, and the electron pair is not shared equally, a bond of two atoms of different elements.

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3
Q

How is the degree of polarity determined?

A

By the difference in electronegativity between the atoms and the symmetry.

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4
Q

What is molecular polarity?

A

The uneven distribution of molecular charge, the existence of both a positive and a negative end of a molecule.

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5
Q

What happens if a molecule contains polar bonds, but is symmetrical?

A

It is non-polar.

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6
Q

Why do multiple covalent bonds occur?

A

Because sometimes to fill up a valence shell of an atom, more than one pair of electrons are needed.

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7
Q

What do compounds containing polyatomic ions have and why?

A

They have both ionic and covalent bonding because the polyatomic ions are held together by polar covalent bonds.

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8
Q

What are coordinate covalent bonds?

A

One atom supplies both electrons for the bond because an ion is attracted to the unshared pair of electrons in a molecule.

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9
Q

What are network solids?

A

Solids in which all of the atoms are covalently bonded to each other, lattice structure.

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10
Q

What are the types of network solids?

A

Diamond - made of carbon
graphite - carbon
silicon dioxide (SiO2)
silicon carbide (SiC)

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11
Q

What is metallic bonding?

A
  • atoms in metal are held together by these
  • the valence electron of a metal atom are held loosely to the atom
  • these electrons are like positive ions
  • all the positive ions share the electrons, creating the electron sea
  • the electrons can move throughout
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12
Q

What does this explain?

A

The malleability and conductivity of metal (because the electrons can move, electricity is conducted).

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13
Q

What holds a molecular covalent substance together in the solid or liquid phase?

A

Attractive/intermolecular forces.

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14
Q

What are the intermolecular forces?

A

dipole-dipole attraction
hydrogen bonding
London dispersion act

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15
Q

What is dipole-dipole attraction?

A

In a polar substance, the positive end of each dipole is attached to the negative end of the next.

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16
Q

What is hydrogen bonding?

A

It is the strongest form of intermolecular attraction, hydrogen bonds form between molecules in which hydrogen is bonded to small atoms having high electronegativity.

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17
Q

What is hydrogen bonding responsible for?

A

unusual properties of water
- water has a relatively high boiling point and low vapor pressure for a small molecule
- water expands when it freezes
- surface tension

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18
Q

What happens when water freezes?

A

The hydrogen bonds hold the molecules in a rigid structure with spaces in between.

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19
Q

Why does surface tension occur?

A

The hydrogen bonding between water molecules in the liquid phase are shared with all neighboring molecules, those on the surface have no neighboring molecules above and therefore, have stronger hydrogen bonds with their nearest neighbors and below the surface.

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20
Q

What are London Dispersion forces?

A

The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles, makes the molecules attracted to each other.

21
Q

What is ion-molecule attraction?

A

The positive ends of water molecules are attracted to the negative salt ions, the negative ends of the water molecules are attracted to the positive salt ions, this disperses the salt into water.

22
Q

What do intermolecular attractions affect?

A

They affect boiling points, melting points, and vapor pressure.

23
Q

What is the relationship between the force of attraction and melting/boiling point?

A

The higher the force of attraction between the particles, the higher the melting/boiling point.

24
Q

What is the relationship between the force of attraction and vapor pressure?

A

The greater the force of attraction, the lower the vapor pressure.

25
Q

How does the force of attraction in ionic compounds compare to the force of attraction in molecular compounds?

A

The force of attraction is stronger in ionic compounds.

26
Q

What are the boiling/melting points of ionic compounds?

A

They are high.

27
Q

What state are ionic compounds usually in at STP?

A

They are usually solid.

28
Q

What state are molecular compounds usually in at STP?

A

They are in liquids or gases.

29
Q

In non polar covalent compounds, what is the relationship between the number of electrons and the force of attraction?

A

The more electrons, the stronger the force of attraction because since there are more electrons, dispersion force is more likely and is stronger, making the compound more polar.

30
Q

What are covalent compounds generally?

A

Non-conductors.

31
Q

What are ionic compounds generally?

A

Non-conductors.

32
Q

Why do ionic solutions conduct electricity?

A

Because of molecule ion attractions, the metal ions are separated, and therefore conduct electricity.

33
Q

What is an atomic orbital?

A

The orbitals of individual atoms.

34
Q

What are molecular orbitals?

A

Orbitals that apply to the entire compound of atoms.

35
Q

Why do atoms bond?

A

To become more stable and lower energy.

36
Q

What are the two types of molecular bonds?

A

Sigma and Pi.

37
Q

What is a sigma bond?

A

Two atomic orbitals combine to form the molecular orbital that is symmetrical along the axes connecting the nuclei. They are single bonds.

38
Q

What are pi bonds?

A

Double and triple bonds. They are likely to be found above and below the bond axis and are weaker than sigma bonds.

39
Q

What do double and triple bonds consist of?

A

One sigma bond and the others are pi bonds.

40
Q

What is hybridization?

A

sp3 hybridization allows a carbon atom to form bonds with 4 other atoms.

41
Q

What is the shape when there is 2 bond pairs and no lone pairs?

A

Linear.

42
Q

What is the shape when there are three bond pairs and no lone pairs?

A

Trigonal planar.

43
Q

What is the shape when there is four bond pairs and no lone pairs?

A

Tetrahedral.

44
Q

What is the shape when there are three bond pairs and 1 lone pair?

A

Trigonal pyramidal.

45
Q

What is the shape when there is 2 bond pairs and 2 lone pairs?

A

Bent.

46
Q

What is the shape when there is 2 bond pairs and 1 lone pair?

A

Bent.

47
Q

What is the shape when there is 6 bond pairs and no lone pairs?

A

Octahedral.

48
Q

what is the shape when there is 5 bond pairs and no lone pairs?

A

Trigonal bipyramidal.

49
Q

What is the shape when there are 2 bond pairs and 1 lone pair?

A

Bent.

Chemistry Honors (11 decks)

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