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My Packs: UWO (CHEM 1301) > Chapter 3: 3.1 Ionic and Covalent Bonding > Flashcards

Chapter 3: 3.1 Ionic and Covalent Bonding Flashcards

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1
Q

True or False:
Only core electrons participate in bonding

A

False, only valence electrons participate in bonding

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2
Q

Elements of low electronegativity typically form:

A

Ionic bonds

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3
Q

Elements of moderate electronegativity typically form:

A

Covalent bonds

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4
Q

Elements of higher electronegativity can form:

A

Covalent or Ionic bonds

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5
Q

True or False:
In an ionic bond, the two atoms share electrons equally

A

False, this is due to the large difference in negativity between the two atoms

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6
Q

When is a bond considered ionic?

A

When there is a complete transfer of an electron from the atom of lower electronegativity to the atom with the higher electronegativity

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7
Q

At what difference in electronegativity do ionic bonds occur?

A

Greater than 1.9

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8
Q

Compounds that have ionic bonds have what properties?

A

High melting points
Crystal lattices

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9
Q

What can Coulomb’s law determine?

A

The magnitude of the attractive force between anions and cations

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10
Q

Scenario:
When ions get bigger, what will happen?

A

Spacing between ions gets bigger
Weaker force of attraction (changes melting points etc.)

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11
Q

Covalent bonds involve _______ of electrons

A

Sharing

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12
Q

True or False:
The electrons in covalent bonds are always shared equally

A

False

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13
Q

At what difference in electronegativity is the sharing of electrons in covalent bonding deemed unequal?

A

Less than 1.9, greater than 0.5

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14
Q

What are covalent bonds with unequal sharing of electrons known as?

A

Polar covalent bonds (Polar bond, for short)

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15
Q

What do polar bonds give rise to?

A

Dipole moment

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16
Q

The greater the difference in electronegativity, the ______ the magnitude of the dipole moment

A

Larger

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17
Q

Dipole moment should be drawn:

A

Either way, as long as you are consistent
Positive to negative (electron pull)
Negative to positive (IUPAC)

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18
Q

What is used to show dipole moment?

A

Electrostatic Potential Maps

19
Q

What do the colors on an Electrostatic Potential Map represent?

A

Red: Negative
Blue: Positive

20
Q

What are covalent bonds with approximately equal sharing of electrons known as?

A

Nonpolar covalent bonds

21
Q

At what difference in electronegativity do nonpolar covalent bonds occur?

A

0.5 or less

22
Q

Why are bonds with an electronegativity difference of 0.5 or lower called “nonpolar covalent bonds”?

A

They have virtually no permanent dipole movements

23
Q

Define:
Lewis structure

A

A diagram showing the atoms, the covalent bonds, the lone electron pairs, and any charges that may be present on the atoms

24
Q

True or False:
Lewis structures show the molecular shape of a molecule

A

False, Lewis structures are not intended to show or imply molecular shape

25
Q

Define:
Formal Charge

A

The difference between the number of electrons “owned’ by that atom in the Lewis structure and the number of valence electrons in a free atom of the same element in its neutral state

26
Q

What is the number of electrons “owned” by an atom?

A

The nonbonding electrons, along with half the electrons in the covalent bonds formed by the atom

27
Q

Define:
Octet Rule

A

If there are enough valence electrons in the molecule, then all of the second-row (2nd row p-block elements) atoms C, N, O, F, Ne must have 8 valence electrons

28
Q

Does the Octet Rule apply to Li and Be? How about B?

A

Li and Be usually do not form covalent bonds, so the Lewis theory is rarely applied to them

Boron-containing compounds usually do not have enough valence electrons for B atoms to satisfy the octet rule

29
Q

True or False:
Atoms in the second row sometimes have more than 8 electrons in a Lewis Structure

A

False, C, N, O, F, and Ne atoms can never have more than 8 electrons in a Lewis structure

30
Q

Lewis Structure Procedure:
Step 1

A

Count total number of valence electrons in molecule by adding valence electrons of each neutral atom
Add one for each negative charge, subtract one for each positive charge

31
Q

Lewis Structure Procedure:
Step 2

A

Draw a skeleton structure, joining atoms together by single bond
Usually element with lowest electronegativity is the central atom

32
Q

Lewis Structure Procedure:
Step 3

A

Count the number of single bonds drawn and calculate the number of valence electrons in the bonds

33
Q

Lewis Structure Procedure:
Step 4

A

Distribute the remaining valence electrons among the atoms

34
Q

Lewis Structure Procedure:
Step 5

A

Assign formal charges to all atoms and check their sum

35
Q

How do we choose the best Lewis structure?

A

The best is normally the structure in which the formal charges are the smallest and consistent with the relative electronegativities of the atoms

36
Q

Define:
Resonance structures

A

Multiple correct Lewis structures that differ only in the positions of the electrons and multiple bonds

37
Q

How are resonance structures best represented?

A

Resonance hybrids

38
Q

Define:
Average bond order

A

Average number of bonds between specific atoms

39
Q

Line Diagrams, True or False:
Each solid line represents an ionic bond

A

False, each solid line represents a covalent bond

40
Q

Line Diagrams, True or False:
If no atom is draw at the intersection of two lines, it is assumed to be a carbon atom

A

True

41
Q

If no atom is drawn at the end of a line, what is it assumed to be?

A

A carbon atom

42
Q

Line Diagrams, True or False:
Hydrogen atoms bonded to carbons are shown

A

False

43
Q

Line Diagrams, True or False:
All non-carbon atoms must be drawn along with hydrogens that are attached to them

A

True

My Packs: UWO (CHEM 1301) (17 decks)

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