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Chemistry 20-1 > Unit 1: Chemical Bonding > Flashcards

Unit 1: Chemical Bonding Flashcards

(56 cards)

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1
Q

What is an energy level?

A

Level of energy around an atom where electrons are found. (1 holds 2, 2 holds 8, 3 holds 8)

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2
Q

What is an orbital?

A

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

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3
Q

What is a valence orbital?

A

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

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4
Q

What are valence electrons?

A

Electrons in the valence orbital

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5
Q

What are bonding electrons?

A

Single electrons in a orbital that bond with electrons in other atoms

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6
Q

What is a lone pair?

A

Two electrons in an orbital

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7
Q

What is electronegativity?

A

The ability of an atom to “hold on”to/ attract

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8
Q

What is the octet rule?

A

A maximum of 8 electrons can occupy the valence level of an atom (elements want to becme close to their nearest noble gas)

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9
Q

What are lewis diagrams?

A

Symbol showing the valence electrons of an atom

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10
Q

What is bonding?

A

Result of two or more atoms fighting for electrons (non metals gains electrons, metals lose)

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11
Q

What helps predict the type of bonding?

A

Electronegativity

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12
Q

What is Covalent Bonding?

A

IF electronegativity of both atoms are high, neither “win” and they share the electron (non metal + non metal)

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13
Q

What is Ionic Bonding?

A

If electronegativities are different >2 then the atom with the higher electronegativity will take the electron (metal + non metal)

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14
Q

How are ionic compounds?

A

They are stable (full valence) and conductive

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15
Q

What are the two types of half reactions?

A
  • reduction
  • oxidation
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16
Q

What is oxidation?

A

The loss of electrons

element = ion + number of electrons lost

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17
Q

What is reduction?

A

Gain of electrons

element + gained electrons + number of atoms

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18
Q

What is net reaction?

A

Combines reduction and oxidation half reactions together

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19
Q

How must the electrons work out in a net reaction?

A

The number of electrons lost in the oxidation half must equal the number of electrons gained in the reduction half

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20
Q

What is molecular bonding?

A

Occursbetween two non-metals

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21
Q

How can molecular bonding be shown?

A
  • Molecular formula
  • Lewis Formula
  • Structural Formula
  • stereochemical formula
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22
Q

What is a molecular formula?

A

Shows all atoms (C2H6)

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23
Q

What is a lewis formula?

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A

uses Lewis symbols (dots)

24
Q

What is a structural formula?

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A

Shows which atoms are bonded using lines

25
What is a stereochemical formua?
Shows the 3D shape
26
How does a stereochemical formula work?
- line = in the plane of the page - wedge = comes forward out of the plane (in front) - dotted lined = goes backward out of the plane (behind)
27
What is bonding capacity?
Max number of bonds that an atom can make (equals number of bonding electrons it has)
28
Hopw do you determine the central atom when drawing lewis diagrams for molecular compounds?
It is the one with the highest bonding capacity
29
How do you draw structural diagrams for molecular compounds?
- start with the lewis diagram - replace every pair of shared electrons with a single line - don't show lone pairs
30
What is stereo chemistry?
The spatial arrangement or 3D distribution of molecules
31
What is VSEPR theory?
Valnce Electron Pair Repulsion Theory; states that pairs of electrons stay as far away from each other as possible
32
What points are true according to VSEPR Theory?
- only the valence electrons of central atoms are important for molecular shape - valence electrons are paired - bonded electron pairs and lone pairs are equal - Electron pairs repel each other - molecular shape is determined when electrons are max distance apart
33
What are the different types of VSEPR Shapes?
- linear - V-shaped - Tetrahedral - Trigonal Pyramid - Trigonal Planar
34
How do you get a linear VSEPR Shape?
- only 2 atoms - central atom bonded to two atoms with no lone pair
35
How do you get a V-Shaped VSEPR Shape?
Central atom has two atoms bonded to it and 1 or 2 lone pairs
36
How do you get a tetrahedral VSEPR Shape?
Central atom has four atoms bonded to it
37
How do you get a trigonal planar VSEPR Shape?
Central atom has three atoms bonded to it and no lone pairs
38
How do you get a trigonal pyramid VSEPR Shape?
Central atom has three atoms bonded to it and one lone pair
39
How do you make a VSEPR Shape?
- draw lewis and structural diagrams - look at central atom and see how many atoms are bonded and how many lone pairs - see the pattern it fits into - draw diagram
40
What ia polarity?
- if two bonded electrons have different electronegativities, they have unequal sharing of the shared pairs of electrons - unequal sharing gives atoms partial charges
41
What is a polar covalent bond?
Covalent bond in which the two bonded atoms have different electronegativity (unequally shared electrons)
42
What is a non-polar covalent bond?
Covalent bond in which the two bonded atoms have the same electronegativity (equally shared electrons)
43
What are bond dipoles?
positive or negative ends of a single molecule
44
What is a polar molecule?
A molecule in which the -ive charge is not distributed symmetrically among the molecule
45
What is a non-polar molecule?
A molecule in which the -ive charge is distributed symmetrically among the molecule
46
How do you determine if a molecule is polar?
- create a VSEPR shape diagram - draw bond dipoles
47
What are intermolecular forces?
Forces between molecules; attract molecules to each other
48
What are intramolecular forces?
Within a molecule (ex. covalent bonding)
49
What are the three types of intermolecular forces and how strong they are?
- London DIspersion (weakest) - Dipole-dipole (middle) - Hydrogen Bonding (strongest)
50
What is London Dispersion force?
Non-polar molecules have a charge of zero but electron movement within a molecule may produce momentary dipole, creating attraction of positive and negative ends - all molecules have London Dispersion force
51
Why does the size of a molecule matter with London Dispersion Force?
The more electrons , the more easily momentary dipoles form, creating a larger force. So larger molecules have more forces.
52
What is Dipole-Dipole Force?
The force of attraction between dipoles of polar molecules - the higher the degree of polarity the stronger the dipole-dipole force
53
What does dipole-dipole determine about solubility?
- like dissolves like - polar molecules dissolve in polar molecules - non-polar molecules dissolve in non-polar molecules
54
What is Hydrogen Bonding?
Force of attraction between a hydrogen bonde3d to O, F, or N of one molecule and the lone pairds of O, F, or N on another molecule - any molecules with -OH or -NH show hydrogen bonding
55
What effect do intermolecular forces have on boiling/melting point?
The higher the intermolecular force the hgiher the melting or boiling point as more forces hold the molecules together
56
What effect do intermolecular forces have on surface tension?
The higher the intermolecular force the higher the surface tension as forces hold surface of liquid intact

Chemistry 20-1 (7 decks)

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