Term
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Definition
| Attractions between atoms |
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Term
| Types of Intramolecular forces |
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Definition
Ionic - positive and negative ions that form a lattice
Covalent - sharing of electrons between atoms
Metallic - electrons shared between closely packed ions |
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Term
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Definition
Attraction between molecules
(Coloumbs law)
F= (Q1 x Q2)/r2
(Size increase, strength increases) |
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Term
| What are Cohesive and Adhesive forces? |
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Definition
Cohesive- between similar molecules
Adhesive- between two different molecules
ex: Cl2-Cl2 cohesive |
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Term
| What are dipole-dipole forces and between which molecules do they occur? |
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Definition
Attraction between positive and negative ends of molecules. only occurs between polar molecules
Gets stronger as dipoles gets bigger |
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Term
| What is Hydrogen bonding and what elements are needed for it to occur? |
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Definition
A strong electronegative element is attracted to a hydrogen connected to another electronegative element on a 2nd molecule.
(F, O, N)=x
x----h-x |
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Term
What are dispersion forces?
What determines the dispersion forces between molecules? |
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Definition
Dispersion forces are temporary dipoles.
occurs in polar and non-polar molecules
larger molecules have larger dispersion forces |
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Term
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Definition
Attraction between Ion and partial charges on a polar molecule.
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Term
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Definition
When a polar molecule induces a dipole in another molecule
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Term
| Strengths of Intramolecular and Intermolecular bonds |
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Definition
Ionic bonds- 600-8000 KJ/mol (Lattice)
Covalent bonds- 100-1100 KJ/mol (bond association)
Intermolecular
ion-ion - 250KJ
Hydrogen bonding - 20KJ
Other forces are small
Inter less then Intra |
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Term
| What forces are broken in Chemical and Physical Changes? |
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Definition
Chemical- Intramolecular forces are broken
Physical- Intermolecular forces are broken
Intermolecular forces intact |
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Term
| Adding heat to a sample increases _______ or ___________. |
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Definition
Kinetic energy- increases temp. uses
q=mc(change in)T
Potential Energy- no change in temp.
occurs at melting and boiling points
energy goes into breaking intermolecular forces
uses (change in)H |
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Term
| Ionic compounds have ______melting points, usually _______celcius |
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Definition
high
thousands of degrees
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Term
| What is the general range of melting points for covalent bonds? |
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Definition
| in the low hundred degrees celcius. |
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Term
| What is an example of Covalent network bonds? |
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Definition
Carbon, graphite or diamond form.
Covalent bonds are prevalant instead of intermolecular bonds. makes melting and boiling points higher. |
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Term
Which has a higher boiling point:
H2S (MW=34) or N2 (MW= 28) |
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Definition
H2S is higher because it is polar. (-60 degrees celcius)
N2 (-196 degrees celcius) |
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Term
| 1 atm = ____kPA = ___ mm Hg = ___ torr= ____psi |
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Definition
| 1 atm = 101kPA = 760 mmHg = 760 torr = 14.7 psi |
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Term
| Properties of an Ideal Gas |
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Definition
Zero volume
behave independently of each other (no attraction or repelling)
Ideal at low pressure, high temperature |
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Term
What is avogardo's law?
Is it a direct or indirect realtionship? |
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Definition
| As moles of gas increases, volume increases. Direct relationship. |
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Term
What is Boyle's law?
Direct or indirect realtionship? |
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Definition
As pressure increases, volume decreases. Same vice versa.
Indirect relationship. |
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Term
| What is the ideal gas law? |
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Definition
PV=nRT
P=pressure
V=Volume
n= moles
R= (0.0821)
T= Temperature |
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Term
What is Charle's law?
direct or indirect? |
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Definition
| As Temperature increases, volume increases. Direct relationship. |
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Term
| What is the Combined Gas Law? |
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Definition
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