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Chemistry 20 > Chapter 3: > Flashcards

Chapter 3: Flashcards

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1
Q

What are structural formulas?

A

Formulas that are more descriptive than chemical formulas because they show us how atoms are bonded together

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2
Q

What is the stability of noble gases related to?

A

The number of electrons in the atom

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3
Q

How can atoms achieve stable electron numbers?

A

By sharing or transferring electrons

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4
Q

What are valence electrons?

A

Electrons in the outermost energy level of an atom

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5
Q

What is an ionic bond explained by?

A

The attraction between positive and negative ions resulting from the transfer of one or more valence electrons

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6
Q

What is a covalent bond explained by?

A

The attraction by the nuclei of atoms for valence electrons that they share between them

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7
Q

Why do only valence electrons matter for bonding?

A

Because electron that are closer to the nucleus are held more tightly and can’t be moved

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8
Q

What is an orbital?

A

A region of space around an atom’s nucleus where an electron may exist

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9
Q

What is a bonding electron?

A

A single electron in a orbital that is available to bond with another electron

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10
Q

What is a lone pair?

A

2 electrons occupying the same orbital

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11
Q

What are lewis symbols?

A

Electron diagrams that represent the number of valence electrons in an atom

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12
Q

What does the element symbol represent in a lewis diagram?

A

It represent the nucleus and all of the non-valence electrons

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13
Q

What is electronegativity?

A

The ability of an atom attract bonding electrons to it valence level

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14
Q

What cause covalent bonding?

A

When the electronegativities are both relatively high neither will win and the bonding electrons will be shared by both atoms

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15
Q

What does ionic bonding depend on?

A

If the electronegativities of 2 atoms have a large difference the atom with the larger electronegativity will take the electron

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16
Q

What is the overall charge on ionic compounds?

A

Neutral because of the way they arrange themselves

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17
Q

What shape do ionic compounds arrange themselves in?

A

A crystal lattice

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18
Q

What is metallic bonding?

A

If both atoms have relatively low electronegativities the atoms share valence electrons because they are not held very strongly by their atoms. The valence electrons act like a sea that holds the positivity

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19
Q

Why are molecular formulas different from ionic formulas?

A

Because they show how the atoms are bonded in molecular formulas

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20
Q

What is bonding capacity?

A

The maximum number of single covalent bonds that an atom can form. It is determined by the number of bonding electrons

21
Q

What is a coordinate covalent bond?

A

When an atom donates 2 electrons to another atom so they both have 8

22
Q

What is a molecular formula?

A

A type of formula that shows how the atoms are bonded. ex. CH3COOH

23
Q

What does a lewis diagram show?

A

It shows how the valence electrons are bonded using dots

24
Q

What does a structural formula show?

A

It uses lines to show how atoms are bonded

25
Q

What is stereochemistry?

A

The study of 3D spatial configuration of molucules

26
Q

What does VSEPR stand for?

A

Valence Shell Electron Pair Repulsion Theory

27
Q

What is VSEPR theory based on?

A

The electrical repulsion of bonded and unbonded pairs in a molecule that aim to stay as far apart as possible

28
Q

What do 2 bond pairs and 0 lone pairs form?

A

Linear

X - A - X

29
Q

What do 3 bond pairs and 0 lone pairs form?

A 
Trigonal Planar
        X
         l
        A
      /     \
   X         X
30
Q

What do 4 bond pairs 0 lone pairs form?

A 
Tetrahedral   
     X
         l
        A
      E   |  \
   X    W   X
31
Q

What do 3 bond pairs 1 lone pair form?

A 
Trigonal Pyramid
            A
         /   |    \
       /     |       \
     X      W     X
32
Q

What do 2 bond pairs and 2 lone pairs form

A

Angular

33
Q

What does 1 bond pairs and 3 lone pairs form?

A

Linear

34
Q

How is the rate that hydrocarbons react affected by bonds?

A
  • Hydrocarbons with multiple bonds react very quickly

- Hydrocarbons with single bonds react slowly

35
Q

What is a polar molecule?

A

A molecule in which the negative charge is not distributed evenly

36
Q

What are the polar molecules?

A
  • Different atoms together
  • Nitrogen and other atoms
  • Oxygen and other atoms
  • Carbon and two other kinds of atoms
37
Q

What are the non-polar molecules?

A
  • All elements

- Containing carbon and one type of other molecule

38
Q

When will a nonpolar covalent bond be formed?

A

When 2 atoms have the same electronegativity so they share electrons equally

39
Q

When will atoms form a polar covalent bond?

A

When they have different electronegativities and do not share electrons equally

40
Q

What is a bond dipole?

A

The charge separation that occurs when there is an electronegativity difference

41
Q

What are intermolecular forces?

A

The forces of attraction and repulsion between molecules

42
Q

What are intramolecular forces?

A

The forces within a molecule

43
Q

What are the 2 Van Der Waals forces?

A

Dipole-Dipole force

London Force

44
Q

What are dipole-dipole forces?

A

Attraction between the positive and negative ends of polar molecules. They are very weak

45
Q

What are london forces?

A

Momentary dipole-dipole forces that occur when electron distribution is momentarily uneven

46
Q

How are electrons and boiling points related?

A

The lesser amount of electrons means the lower boiling point because it is easier to separate bonds

47
Q

What is hydrogen bonding?

A

An intermolecular force when a hydrogen nucleus could be shared between electrons on adjacent molecules

48
Q

What three atoms can be used in hydrogen bonding?

A

Nitrogen
Oxygen
Fluorine

Chemistry 20 (10 decks)

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