Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
41 Cards in this Set
- Front
- Back
Chemical Evolution
|
Simple chemical compounds in the atmosphere & oceans combined to form larger and more complex molecules, which led to the origin of life
|
|
What two major events happened as the Earth began to cool?
|
1. Water rained out of the atmosphere to form the first ocean
2. Many volcanoes existed, which spewed volcanic gas into the atmosphere |
|
What is the important characteristic of the outer-most shell of the valence electrons?
|
The number of unpaired electrons (or valence) is very important for chemical bonding patterns.
|
|
Describe covalent bonding patterns
|
Valence electrons are shared between 2 atoms, which bind together to form molecules; equal sharing forms non-polar molecules/ unequal = polar.
|
|
Electronegativity
|
The degree with which atom's share their valence electrons in covalent bonds.
|
|
Describe ionic bonds
|
Valence electrons are completely transferred from one atoms to another; ions form, bonding them together.
|
|
What is the difference between cations and anions?
|
Cations- Positively charged ions
Anions- Negatively charged ions |
|
In a molecule, what dicates the behavior and function?
|
The overall shape (bond angles).
|
|
Molecular Formula
|
The number and type of atoms in a molecule.
|
|
Structural Formula
|
Which atoms are bonded together; single, double, and triple bonds are shown by single, double, and triple dashes.
|
|
Molecular Weight
|
The sum of the mass numbers of all the atoms in a molecule.
|
|
Molarity
|
The number of moles of a substance per Liter.
|
|
Chemical Reaction
|
An event in which one substance is combined with others or broken down into another substance.
|
|
T/F Changing the concentration of the reactants or of the products can disturb the chemical equilibrium.
|
True.
|
|
Eplain the difference between endo and exothermic reactions.
|
Endothermic- Heat is absorbed in the chemical process; driven to right
Exothermic- Heat is released; equilibrium driven to left. |
|
Energy
|
The capacity to do work or supply heat; exists either as stored potential energy or active motion.
|
|
Thermal Energy
|
The kinetic energy of molecular motion.
|
|
Temperature
|
The measure of how much thermal energy its molecules pocess.
|
|
Heat
|
The transferrence of thermal energy from one molecule to another.
|
|
What happens when an electron 'falls' into a lower electron shell?
|
It experiences a loss of potential energy because it uses some it its kinetic energy in the fall.
|
|
First Law of Thermodynamics
|
Energy is converted from one form to another; it can neither be created or destroyed.
|
|
Second Law of Thermodynamics
|
Entropy always increases in a closed system.
|
|
Chemical Energy
|
The potential energy stored in chemical bonds.
|
|
What makes reactions spontaneous?
|
1. Products have lower potential energy than reactants (exothermic) (H)
2. Products are less ordered than reactants (increased entropy) (S) |
|
Gibbs Free-energy change
|
Delt G = Delta H - T Delta S, where T stands for the temperature in Kelvin; if G is greater than 0, the reaction is non-spontaneous; if 0, there is equilibrium.
|
|
Why is sunlight important for the theory of chemical evolution?
|
Energy from photons can break molecules apart by knocking electrons out of the outer shell of atoms.
|
|
Free Radicals
|
The resulting atoms, which have unpaired electrons and are extremely unstable.
|
|
What 2 things can speed up reaction times?
|
1. Higher temperature
2. Greater concentration |
|
Explain the difference between reducton and oxidation.
|
Reduction is the gaining of an electron and oxidation is the loss of an electron; OIL RIG --> Oxidation is loss, Reduction is gain (often adding/losing Hs)
|
|
Why does water have such a high specific heat?
|
It takes an extraordinarily large amount of energy to break the hydrogen bonds.
|
|
Specific Heat
|
The amount of energy required to raise the temperature of a substance by 1 degree Celcius
|
|
Explain the difference between acids and bases
|
Acids give up a proton during chemical reactions; Bases acquire a proton during chemical reactions
PH is determined by -log[H+] |
|
Air (dry)
|
1.01
|
|
Aluminum
|
.90
|
|
Cooper
|
.39
|
|
Gold
|
.13
|
|
Iron
|
.45
|
|
Mercury
|
.14
|
|
Table Salt
|
.86
|
|
Water (s)
|
2.03
|
|
Water (l)
|
4.18
|