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Chemistry 1010 Test 4 Flashcards | StudBud
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Chemistry 1010 Test 4
Chemistry 1010 Test 4
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1
Volume (V)
When gas (force) strike the walls of their container, they exert pressure.
Pressure exerted by column of air from top of atmosphere to surface.
Equals the size of the container in which the gas is placed.
2
Temperature & Pressure (Gay-Lussac’s Law)
P₁V₁ = P₂V₂
P₁/T₁ = P₂/T₂
V₁/T₁ = V₂/T₂
3
Pressure & Volume (Boyle’s Law)
P₁/T₁ = P₂/T₂
P₁V₁ = P₂V₂
V₁/T₁ = V₂/T₂
4
Electronegativity
Bonding e- are shared unequally.
Polar or non-polar.
Bonding e- are shared equally.
The relative ability of atoms to attract shared electrons.
5
Shared Electrons (bonding pairs)
A convenient way to represent the valence electrons.
Placed on the outside of the element.
Shown as 2 dots or a single line of atoms.
6
Electronic Shape
Placing e- groups as far apart as possible around the central atom.
Number of electron groups surrounding central atom.
Number of atoms bonded to central atom.
7
Valence Shell Electron-Pair Repulsion (VSEPR)
Placing e- groups as far apart as possible around the central atom.
Number of electron groups surrounding central atom.
Number of atoms bonded to central atom.
8
Dispersion Forces
Strong dipole-dipole attractions.
Very weak attractive forces that occur between non-polar molecules.
9
1. Dipole-Dipole Attractions
Polar H-bonded with N, O, or F).
Polar
Attractive forces between mol. & ions holds close together in liquids/solid
Only in for non-polar compounds.
10
Combined Gas Law
P₁V₁/T₁ = P₂V₂/T₂
PV = nRT … R=gas constant
V₁/n₁ = V₂/n₂
11
Pressure (P)
Pressure exerted by column of air from top of atmosphere to surface.
When gas (force) strike the walls of their container, they exert pressure.
Equals the size of the container in which the gas is placed.
12
The Kinetic Molecular Theory of Gases (Pt. 1)
A gas consists of small particles that move randomly w/ high velocities.
Actual vol. occupied by gas mol. is small compared to vol. the gas occupies
The attractive forces between the particles of a gas are usually small.
13
Temperature & Volume (Charles’s Law)
P₁V₁ = P₂V₂
V₁/T₁ = V₂/T₂
Tc+273=Tk
P₁/T₁ = P₂/T₂
14
Polar Covalent (𝛿⁻ OR 𝛿⁺)
1.9 - 3.3
0.0 - 0.4
0.5 - 0.8
15
3. Dispersion Forces
Polar
Attractive forces between mol. & ions holds close together in liquids/solid
Polar H-bonded with N, O, or F).
Only in for non-polar compounds.
16
Double Bond
2 pairs of electrons are shared.
Forms when there aren’t enough valence electrons to complete octets.
3 pairs of electrons are shared.
1 pair of electrons is shared.
17
Ionic compounds that…
Do not dissolve in water are insoluble salts
Dissolve in water are soluble salts
18
Triple Bond
3 pairs of electrons are shared.
Forms when there aren’t enough valence electrons to complete octets.
1 pair of electrons is shared.
2 pairs of electrons are shared.
19
Solubility
The maximum amount of solute that dissolves in a specific amount of solvent
Matter
=g of water/100 g water
20
Atmospheric Pressure (atm)
Equals the size of the container in which the gas is placed.
When gas (force) strike the walls of their container, they exert pressure.
Pressure exerted by column of air from top of atmosphere to surface.
21
Boiling Point of Water…
Higher at higher pressures.
Pressure above a liquid at equilibrium in a closed container.
Depends on the vapor pressure.
At sea level 1 atm=760 mmHg
22
Non-Polar Covalent
0.5 - 0.8
0.0 - 0.4
1.9 - 3.3
23
The Ideal Gas Law
P₁V₁/T₁ = P₂V₂/T₂
R=0.0821 L x atm/moles x K
V₁/n₁ = V₂/n₂
PV = nRT … R=gas constant
24
The Kinetic Molecular Theory of Gases (Pt. 2)
The average kinetic energy of gas mol. is proportional to the K temp.
Gas particles are in constant motion, moving rapidly in straight paths.
25
3 Electron Groups
Linear electron-group geometry.
Linear shape with a bond to minimize repulsion.
Trigonal planar shape with a bond to minimize repulsion.
Trigonal planar electron geometry.
26
Vapor Pressure
At sea level 1 atm=760 mmHg
Pressure above a liquid at equilibrium in a closed container.
Depends on the vapor pressure.
Higher at higher pressures.
27
4 Electron Groups
Trigonal planar electron geometry.
Trigonal planar shape with a bond to minimize repulsion.
Tetrahedral shape with a bond to minimize repulsion.
Tetrahedral electron-group geometry.
28
2. Hydrogens Bonding
Polar
Attractive forces between mol. & ions holds close together in liquids/solid
Polar H-bonded with N, O, or F).
Only in for non-polar compounds.
29
Hydrogen Bonds
Very weak attractive forces that occur between non-polar molecules.
Strong dipole-dipole attractions.
30
Henry’s Law
Depends on the temperature
Decreases as temperature increases for gases
Increases as temperature increases for most solids.
When pressure of gas above sol. decreases, solubility of gas also decreases
31
Solutes aren’t visible &…
Cannot be separated by filteration.
Can give color to a solution.
Can be separated by evaporation.
“Like dissolves like” … BOTH POLAR OR BOTH NON-POLAR
32
Lewis Structure
A convenient way to represent the valence electrons.
Shown as 2 dots or a single line of atoms.
Placed on the outside of the element.
33
Atmospheric Pressure (atm)
1 atm=760 torr.
Tc+273=Tk
1 mmHg=1 torr.
1 atm=760 mmHg
34
Strong Electrolytes
Conduct an electric current
Produce ions
Produce a few ions
Completely dissociates (break up)
35
Ionic (+ OR -)
0.5 - 0.8
0.0 - 0.4
1.9 - 3.3
36
Non-Polar Covalent Bonds
The relative ability of atoms to attract shared electrons.
Bonding e- are shared equally.
Polar or non-polar.
Bonding e- are shared unequally.
37
Solvent
Usually present in greater quantity.
Homogeneous mixtures of 2 or more substances.
Smaller quantity, and dissolved in another substance.
38
Intermolecular Force
Polar
Only in for non-polar compounds.
Polar H-bonded with N, O, or F).
Attractive forces between mol. & ions holds close together in liquids/solid
39
Polar Covalent Bonds
Bonding e- are shared equally.
Polar or non-polar.
Bonding e- are shared unequally.
The relative ability of atoms to attract shared electrons.
40
Weak Electrolytes
Do not produce ions
Dissolve mostly as molecules
Conduct a weak current
Produce a few ions
41
Single Bond
3 pairs of electrons are shared.
Forms when there aren’t enough valence electrons to complete octets.
2 pairs of electrons are shared.
1 pair of electrons is shared.
42
Solute-Solvent Attractions
Most common polar solvent= WATER
Can give color to a solution.
Most common non-polar solvent= HEXTNE
“Like dissolves like” … BOTH POLAR OR BOTH NON-POLAR
43
Solute
Homogeneous mixtures of 2 or more substances.
Smaller quantity, and dissolved in another substance.
Usually present in greater quantity.
44
2 Electron Groups
Trigonal planar electron geometry.
Linear shape with a bond to minimize repulsion.
Linear electron-group geometry.
Trigonal planar shape with a bond to minimize repulsion.
45
Multiple Bonds
Forms when there aren’t enough valence electrons to complete octets.
1 pair of electrons is shared.
2 pairs of electrons are shared.
3 pairs of electrons are shared.
46
Volume & Moles (Avogadro’s Law)
P₁V₁/T₁ = P₂V₂/T₂
PV = nRT … R=gas constant
V₁/n₁ = V₂/n₂
47
Molecular Shape
Placing e- groups as far apart as possible around the central atom.
Number of atoms bonded to central atom.
Number of electron groups surrounding central atom.
48
Nonelectrolytes
Do not conduct a current
Do not produce ions
Dissolve as molecules
Produce ions
49
Solutions
Homogeneous mixtures of 2 or more substances.
Smaller quantity, and dissolved in another substance.
Usually present in greater quantity.
50
Non-bonding Pairs (lone pairs)
Shown as 2 dots or a single line of atoms.
Placed on the outside of the element.
A convenient way to represent the valence electrons.
51
When electrolytes dissolve in water…
“Like dissolves like”
Completely dissociate into ions, forming a solution that conducts elect.
52
Solubility
Depends on the temperature
Decreases as temperature increases for gases
Increases as temperature increases for most solids.
When pressure of gas above sol. decreases, solubility of gas also decreases
53
Resonance Structures
Are shown with a double-headed arrow.
May be written for molecules with multiple bonds.
Consists of 2+ electron-dot formulas for same arrangement of atoms.
Written by changing the location of a double bond.
