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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. |
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| Formula for calculating number of moles from number of particles |
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Definition
n=(N)/(Avogadro's Constant) |
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Definition
| Mass of an element in a compound expressed as a percent of the total mass of the compound. |
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Term
| Dilution (helpful formula) |
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Definition
When you dilute a solution, you can use the following formula to dtermine the new molarity Molarity=M, Volume = V M1V1=M2V2 |
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Definition
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Term
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Definition
| Substance being dissolved |
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Definition
| The number of particles in one mole (6.02 * 10^23) |
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Definition
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Term
| Bronsted-Lowry definition of acids and bases |
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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 |
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Definition
PV=nRT Where: R= about 8.314 |
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Term
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Definition
| Degree to which two liquids can mix in a homogeneous fashion |
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Term
| Dipole-Dipole attractions |
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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. |
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Term
Find the conjugate acid/base pair in this reaction: CH3COOH (arrows pointing back and forth) H+ (aq) + CH3COO- |
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Definition
| CH3COOH is the conjugate acid and CH3COO- is the conjugate base |
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Term
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Definition
| The relative mass of each element in a compound. |
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Term
| Kinetic molecular theory of gases (give the whole rule) |
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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 |
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Definition
| Relative amount in which each isotope is present in a given sample of an element. |
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Term
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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. |
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Term
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Definition
| The species reduced because it causes the other species to give up electrons |
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Definition
| The mass of one mole of a substance |
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Term
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Definition
| Substance dissolving the solute |
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Term
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Definition
| Simplest formula, where all the subscripts are reduced to the simplest form. For example, |
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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? |
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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 |
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Term
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Definition
| Solvent + dissolved solute |
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Term
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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. |
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Definition
| A hydrocarbon with a carbon-carbon double bond |
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Term
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Definition
| Number of acid equivalents = # of base equivalents |
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Term
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Definition
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Term
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Definition
| # moles of solute per L of solvent |
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Term
| % composition by mass in solutions |
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Definition
| In solutions, you can just divide the weight of the solute by the weight of the solution to find the % composition by mass. |
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Term
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Definition
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| Arrhenius Definition of Acids and Bases |
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Definition
Acids are a species producing H+ in an aqueous solution. Bases are a species producing OH- in an aqueous solution. |
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Term
| Formula for perchloric acid |
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Definition
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Term
| Law of definite proportions |
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Definition
| the elements in a chemical compound are always present in the same proportions by mass |
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Definition
| Weighted average of all the masses of the isotopes of the element adjusted for abundance |
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Term
| Formula for determining pH and formula for determining pOH |
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Definition
pH=-log[H+]=log(1/[H+]) pOH= -log [OH-] |
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Term
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Definition
| Wehn an atom LOSES electrons |
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Term
| Dalton's Law of Partial Pressures |
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Definition
| P(t)=P(1)+P(2)+P(3)...... |
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Term
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Definition
| When an electron GAINS electrons |
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Term
| Oxidation number of Cl in HOCl |
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Definition
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Term
| How many F are required for the reduction of 1 mol of Ni2+ to Ni (s) |
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Definition
| 2 F, because 2 moles of electrons are required |
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