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test 1
lectures and more
23
Chemistry
Not Applicable
02/13/2006

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Term
Intramolecular forces
Definition
Attractions between atoms
Term
Types of Intramolecular forces
Definition
Ionic - positive and negative ions that form a lattice
Covalent - sharing of electrons between atoms
Metallic - electrons shared between closely packed ions
Term
Intermolecular forces
Definition
Attraction between molecules
(Coloumbs law) F= (Q1 x Q2)/r2
(Size increase, strength increases)
Term
What are Cohesive and Adhesive forces?
Definition
Cohesive- between similar molecules
Adhesive- between two different molecules
ex: Cl2-Cl2 cohesive
Term
What are dipole-dipole forces and between which molecules do they occur?
Definition
Attraction between positive and negative ends of molecules. only occurs between polar molecules
Gets stronger as dipoles gets bigger
Term
What is Hydrogen bonding and what elements are needed for it to occur?
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
Term
What are dispersion forces?
What determines the dispersion forces between molecules?
Definition
Dispersion forces are temporary dipoles.
occurs in polar and non-polar molecules
larger molecules have larger dispersion forces
Term
Ion-Dipole forces
Definition
Attraction between Ion and partial charges on a polar molecule.
Term
Dipole-Induced Dipole
Definition
When a polar molecule induces a dipole in another molecule
Term
Strengths of Intramolecular and Intermolecular bonds
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
Term
What forces are broken in Chemical and Physical Changes?
Definition
Chemical- Intramolecular forces are broken
Physical- Intermolecular forces are broken
Intermolecular forces intact
Term
Adding heat to a sample increases _______ or ___________.
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
Term
Ionic compounds have ______melting points, usually _______celcius
Definition
high
thousands of degrees
Term
What is the general range of melting points for covalent bonds?
Definition
in the low hundred degrees celcius.
Term
What is an example of Covalent network bonds?
Definition
Carbon, graphite or diamond form.
Covalent bonds are prevalant instead of intermolecular bonds. makes melting and boiling points higher.
Term
Which has a higher boiling point:
H2S (MW=34) or N2 (MW= 28)
Definition
H2S is higher because it is polar. (-60 degrees celcius)
N2 (-196 degrees celcius)
Term
1 atm = ____kPA = ___ mm Hg = ___ torr= ____psi
Definition
1 atm = 101kPA = 760 mmHg = 760 torr = 14.7 psi
Term
Properties of an Ideal Gas
Definition
Zero volume
behave independently of each other (no attraction or repelling)
Ideal at low pressure, high temperature
Term
What is avogardo's law?
Is it a direct or indirect realtionship?
Definition
As moles of gas increases, volume increases. Direct relationship.
Term
What is Boyle's law?
Direct or indirect realtionship?
Definition
As pressure increases, volume decreases. Same vice versa.
Indirect relationship.
Term
What is the ideal gas law?
Definition
PV=nRT
P=pressure
V=Volume
n= moles
R= (0.0821)
T= Temperature
Term
What is Charle's law?
direct or indirect?
Definition
As Temperature increases, volume increases. Direct relationship.
Term
What is the Combined Gas Law?
Definition
(P1V1)/T1= (P2V2)/T2
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