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Chemistry 20 > Chapter 3: Notes > Flashcards

Chapter 3: Notes Flashcards

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1
Q

What do structural formulas show?

A

The way in which atoms are bonded together

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2
Q

What causes a chemical bond?

A

The attraction of electrons by two atomic nuclei. the nucleus of its own atom and another atom

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3
Q

What are valence electrons?

A

The electrons that occupy the outermost energy level

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4
Q

What are the places that electrons exist in called?

A

Orbitals

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5
Q

What is an orbital?

A

A region of space where there is a high probability of finding electrons of a particular energy

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6
Q

How many electrons can an orbital be occupied by?

A

one or two electrons

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7
Q

What is a bonding electron?

A

A single electron occupying an orbital

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8
Q

What is a lone pair?

A

Two electrons occupying a filled orbital (non-bonding)

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9
Q

what determines an atoms bonding capacity?

A

The maximum number of bonding electrons

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10
Q

What is bonding capacity?

A

The number of covalent bonds formed by an atom

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11
Q

What is electronagativity?

A

The tendancy for an atom to attract electrons to itself (from other atoms) when is is chemically combined with another element

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12
Q

How is electronegativity organized in the periodic table?

A

It increases from left to right

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13
Q

What are covalent bonds?

A

They involve atoms sharing of a pair of electrons to get a full (8 electron) outer shell

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14
Q

What is ionic bonding?

A

When electrons are transferred from metals (low electronegativity) to non-metals (high electronegativity)

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15
Q

What is the result of ionic bonding?

A

The formation of positive cations and negative anions

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16
Q

What is an example of an empirical chemical formula?

A

A regular formula CH(sub)2O

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17
Q

What is an example of a molecular formula?

A

CH3OOH The h’s are separated

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18
Q

What is an example of a Lewis formula?

A

A dot diagram

19
Q

What is an example of a structural formula?

A

the line diagrams

20
Q

What is an example of the stereochemical formulas?

A

The ones that show the depth

21
Q

How do you draw the Lewis formula for polyatomic ions?

A

You add 1 extra electron for every negative charge

22
Q

What does VSEPR stand for?

A 
Valence
Shell
Electron
Pair
Repulsion
23
Q

What is important for molecular shape?

A

The valence electrons of the central atoms

24
Q

What is the molecular shape determined by?

A

The positions of the electron pairs when they are the maximum distance apart

25
Q

How do valence electrons repel each other?

A

Electrostatically

26
Q

What repels more strongly: Lone pairs or bond pairs?

A

Lone pairs!

27
Q

What does 2 bond pairs and 0 lone pairs form?

A

Linear H - Be - H

28
Q

What does 3 bond pairs and 0 lone pairs form?

A 
AX3 Triagonal planar
          H
           l
          B
        /     \
  H           H
29
Q

What do 4 bond pairs and 0 lone pairs form?

A

AX4 Tetrahedral. 2 at level one below one on top

30
Q

What do 3 bond pairs and 1 lone pair form?

A

AX3E tetrahedral. 1 below one above and one at level

31
Q

What do 2 bond pairs and 2 lone pairs?

A

AX2E2 tetrahedral V shaped

32
Q

What does 1 bond pair and 2 lone pairs create?

A

AXE3. Linear

33
Q

What are polar molecules?

A

Molecules that have one end that is slightly negative and one end that is slightly positive

34
Q

what does bond polarity depend on?

A

The elctronegativities of the bonded atoms

35
Q

When are covalent bonds polar?

A

when the atoms have dfferent negativities

36
Q

Which side of an atom is labelled as partially negative?

A

The side of the atom where the electron spends more time which is around the nucleus with higher electronegativity

37
Q

When is a covalent bond non-polar?

A

When there is no difference in electronegativity ex H-H

38
Q

When is a covalent bond slightly polar?

A

When the difference of electronegativity is between 0.1 - 1.0 ex H -Cl

39
Q

When is a covalent bond very polar?

A

When the difference of electronegativity is between 1.1 - 2.0 H - F

40
Q

When is a bond ionic?

A

When the difference in electronegativity is greater than 2.1

41
Q

What is the bond dipole?

A

The charge separation that occurs as a result of the different electronegativities of bonded atoms

42
Q

What is the bond dipole represented by?

A

An arrow that points from lower to higher electronegativity

43
Q

What happens in non polar molecules with a bond dipole?

A

the bond dipoles cancel out, leaving a molecular dipole of 0 ex. CO2

44
Q

Why are molecules that are symetrical non-polar?

A

Becuase the dipole moments balance

Chemistry 20 (10 decks)

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