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Stoichiometry and Other Misc
11th Grade Final Exam
40
Chemistry
11th Grade
06/10/2008

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Term
Hydrogen Bonding
Definition
A specific bond which occurs only between hydrogen and other, fairly electronegative atoms. When Hydrogen bonds to a very electronegative atom, like Fluorine, it basically loses its electron and so it becomes very positively charged. It now interacts strongly with the negatively charged sides of other electronegative atoms.
Term
Formula for calculating number of moles from number of particles
Definition

n=(N)/(Avogadro's Constant)

Term
Mass percent
Definition
Mass of an element in a compound expressed as a percent of the total mass of the compound.
Term
Dilution (helpful formula)
Definition

When you dilute a solution, you can use the following formula to dtermine the new molarity

Molarity=M, Volume = V

M1V1=M2V2 

Term
Boyle's Law
Definition
p1v1=p2v2
Term
Solute
Definition
Substance being dissolved
Term
Avogadro's constant
Definition
The number of particles in one mole (6.02 * 10^23)
Term
Charle's Law
Definition
V(1)/T(1)=V(2)/T(2)
Term
Bronsted-Lowry definition of acids and bases
Definition
According to Bronsted-Lowry, acids donate protons and bases accept protons. These acids and bases always occur in pairs, and the second substance in a pairing is called the conjugate acid/base
Term
Ideal Gas Law
Definition

PV=nRT

Where:

R= about 8.314 

Term
Miscibility
Definition
Degree to which two liquids can mix in a homogeneous fashion
Term
Dipole-Dipole attractions
Definition
When polar molecules orient themselves such that their positive ends are closer to the negative ends of the other particles. This produces higher boiling points than comparable non-polar intermolecular forces. Dipole-Dipole rarely occurs in the gaseous phase because the atoms are so far apart.
Term

Find the conjugate acid/base pair in this reaction:

 

CH3COOH (arrows pointing back and forth) H+ (aq) + CH3COO-

Definition
CH3COOH is the conjugate acid and CH3COO- is the conjugate base
Term
Percent composition
Definition
The relative mass of each element in a compound.
Term
Kinetic molecular theory of gases (give the whole rule)
Definition

The theory defining the conditions for an "ideal gas":

1) Gases are made of particles whose size is negligible in comparison to the size of their container

2) Gas atoms or molecules do not show any significant intermolecular attraction or repulsion

3) Gas particles are in continuous and random motion, colliding with other particles and the container wall

4) Collisions between any gas particles are elastic, so no energy is dissipated

5) The average kinetic energy of gas particles is proportional to the absolute temperature of the gas, and is the same for all gases at that temperature 

Term
Isotopic abundance
Definition
Relative amount in which each isotope is present in a given sample of an element.
Term
Isotope
Definition

An atom with the same number of protons as a normal atom of that element but a different number of neutrons

For example, one of Hydrogen's isotopes, deutirium, has an atomic weight of 2 but only 1 proton, meaning one neutron has been added to the hydrogen. It is still called hydrogen because of the number of protons.  

Term
Oxidation agent
Definition
The species reduced because it causes the other species to give up electrons
Term
Molar mass
Definition
The mass of one mole of a substance
Term
Solvent
Definition
Substance dissolving the solute
Term
Empirical formula
Definition
Simplest formula, where all the subscripts are reduced to the simplest form. For example,
Term
What is the molar mass of a 2.8 g sample of gas that occupies a volume of 3L at a temperature of 546 K and pressure 1.5 atm?
Definition

Volume@STP= 3L (original volume) *(273 K/546 K) * (1.5 atm/1 atm)

Volume @ STP = 2.25 L

2.8g/2.25 L = 1.24 g/L (this is the density) at STP

molar mass= 1.24 g/L * 22.4 L/mol = 28 g/mol

NOTE the 22.4 comes from the rule that one mol of any gas will occupy 22.4 L at STP

The sample is most likely N2

Term
Solution
Definition
Solvent + dissolved solute
Term
Saturation
Definition
When no more solute can be dissolved into the solvent. For example, if one is dissolving sugar into boiling water, the water will be saturated when the sucrose remains in the solid phase and sinks to hte bottom of the container.
Term
Definition of an alkene
Definition
A hydrocarbon with a carbon-carbon double bond
Term
Equivalence point
Definition
Number of acid equivalents = # of base equivalents
Term
Mass of carbon-12 in amu
Definition
12
Term
Molarity
Definition
# moles of solute per L of solvent
Term
% composition by mass in solutions
Definition
In solutions, you can just divide the weight of the solute by the weight of the solution to find the % composition by mass.
Term
ATP in torr
Definition
760
Term
Arrhenius Definition of Acids and Bases
Definition

Acids are a species producing H+ in an aqueous solution.

Bases are a species producing OH- in an aqueous solution.

Term
Formula for perchloric acid
Definition
HClO4
Term
Law of definite proportions
Definition
the elements in a chemical compound are always present in the same proportions by mass
Term
Average atomic mass
Definition
Weighted average of all the masses of the isotopes of the element adjusted for abundance
Term
Formula for determining pH and formula for determining pOH
Definition

pH=-log[H+]=log(1/[H+])

pOH= -log [OH-]

Term
Oxidation
Definition
Wehn an atom LOSES electrons
Term
Dalton's Law of Partial Pressures
Definition
P(t)=P(1)+P(2)+P(3)......
Term
Reduction reaction
Definition
When an electron GAINS electrons
Term
Oxidation number of Cl in HOCl
Definition
+1 (EXCEPTION)
Term
How many F are required for the reduction of 1 mol of Ni2+ to Ni (s)
Definition
2 F, because 2 moles of electrons are required
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