Chemistry Flashcards
Scientific notation:
Scientific system of writing numbers
Scientific notation is composed of 3 parts:
- a mathematical sign (+ or -)
- Significand
- Exponential/logarithm
Basic measurements of the metric system:
Grams (weight)
Liters (volume)
Meters (distance)
3 common temperature systems:
Fahrenheit, Celsius, Kelvin
Fahrenheit:
A. Zero degrees (0 F) is the freezing point of sea water at sea level
B. 32 F is the freezing point of pure water at sea level
C. 212 F is the boiling point of pure water at sea level
Celsius:
A. Zero degrees (0 C) is the freezing point of pure water at sea level
B. 100 C is the boiling point of pure water at sea level
C. Most people have a body temp of 37 C
Kelvin:
A. Zero degrees (0 K) is -273.15 C and is the lowest temp achievable or absolute zero
B. The freezing point of water is 273 K
C. The boiling point of water is 373 K
Atom is composed of:
Protons and neutrons in the center and electrons orbiting the outside
The electrons orbit the nucleus at various energy levels called:
Shells or orbits
Charge of protons, electrons, neutrons:
Proton (+)
Electron (-)
Neutron (no charge)
When an atom is electrically charged, it’s called:
Ion
Cation:
Atom that has a positive charge
Anion:
Atom that has a negative charge
Rows in a periodic table are called:
Periods
Columns in a periodic table are called:
Groups
Atomic number:
Number or protons in the nucleus
Atomic mass:
The average mass of each of that element’s isotopes
Isotope:
Different kinds of the same atom that vary in weight
Compound:
Combination of atoms and other elements
Law of conservation of mass states:
Mass cannot be created or destroyed during a chemical reaction. Therefore, the equation must be rearranged and balanced.
Equilibrium:
A state in which reactants are forming products at the same rate that products are forming reactants (reversible).
4 ways to increase reaction rate:
- Increase in temp
- Increase in surface area of reactants
- Add a catalyst
- Increase concentration of reactants
Increasing the temp causes:
Particles to have a great kinetic energy that causes them to move around so fast that they collide
Increasing the surface area causes:
More opportunity for the particles to come in contact with one another
Adding a catalyst:
Reduces the activation energy or amount of energy necessary for a reaction to occur
Examples of catalyst:
Metals and proteins (enzymes)
Increasing the concentration causes:
More chance of collisions between the reactants, which produces more products
Solution:
Homogenous mixture of two or more substances
Solute:
Parts being dissolved
Solvent:
Part doing the dissolving
4 types of solutions:
- Compounds
- Alloys
- Amalgams
- Emulsions
Alloys:
Solid solution of metals to make a new one (Ex. copper + tin= bronze)
Amalgams:
A specific type of alloy in which a metal is dissolved in mercury
Emulsions:
Mixtures of matter that readily separate such as water and oil
Concentration is expressed as:
Weight per weight
Weight per volume
Volume per volume
A mole is:
AKA
6.02 x 10^23
Avogadro’s number
5 types of chemical reactions:
- Synthesis
- Decomposition
- Combustion
- Single replacement
- Double replacement
Synthesis:
Two elements combine to form a product
Decomposition:
Opposite of synthesis- breaking of a compound into its compound parts
Combustion:
Self-sustaining exothermic chemical reaction where oxygen and a fuel compound react
Single replacement:
Consist of an active metal reacting with an ionic compound containing a less active metal to produce a new compound
Double replacement:
- Involves two ionic compounds: the positive ion from one compound combines with the negative ion of the other compound
- “Switching partners”
2 types of chemical bonding:
Ionic and covalent
Ionic bonding:
- Electrostatic attachment between two oppositely charged ions (or a cation and an anion)
- Formed between metal and nonmetal
Covalent bonding:
- Formed when two atoms share a pair of electrons with one pair from each atom
- Formed between two nonmetals
- Strongest bond
Non-polar bond:
Electrons in a covalently bonded compound are shared equally
Polar bond:
The shared electron density is concentrated around one atom more than the other (not equal)
Intermolecular forces:
Weaker forces of attraction between whole molecules
List 3 intermolecular forces:
- Hydrogen bonding
- Dipole-dipole interactions
- Dispersion forces
Hydrogen bond:
- The attraction for a hydrogen atom by a highly electronegative element
- Strongest of all intermolecular forces
Dipole-dipole interactions:
The attraction of one dipole on one molecule for the dipole of another molecule
Dipole:
Separation of charges within a molecule between two covalently bonded atoms
Dispersion forces:
- When the electrons within an element or compound concentrate themselves on one side of an atom causing a temporary dipole
- Weakest of all intermolecular forces
Stoichiometry:
Quantities and numeric relationships of the participants in a chemical reaction
Dimensional analysis:
Process used to determine the number of moles of oxygen needed to complete the reaction
Oxidation:
Loss of electrons
Reduction:
Gain of electrons
OIL-RIG:
Oxidation is loss (of an electron)
Reduction is gain (of an electron)
These elements, when they exist outside of a compound in their natural state, are always in pairs:
Hydrogen, bromine, oxygen, nitrogen, iodine, and fluorine.
Series of rules to identify the oxidation states of all elements in the compound:
- The charge or number of any element in it’s natural state is zero.
- The oxidation number of any simple ion is the charge of the ion
- The oxidation number for oxygen in a compound is (-2)
- The oxidation number for hydrogen in a compound is (+1)
- The sum of the oxidation numbers equals the charge on the molecules or polyatomic ions
Acids:
- Corrosive to metals
- Change blue litmus paper red
- Become less acidic when mixed with bases
- Hydrogen or proton donors
Bases:
- AKA alkaline compounds
- Denature proteins
- Change red litmus paper blue
- Become less basic when mixed with acids
- Hydrogen or proton acceptors
Chemical reactions:
Atoms are trying to reach stable electron configurations
Nuclear reactions:
Concerned with reactions that take place in the nucleus to obtain stable nuclear configurations
Radioactivity:
The emission of particles and/or energy (radiation) from an unstable nucleus
3 types of radiation in nuclear chemistry:
Alpha, beta, gamma
Alpha radiation:
- Emission of helium nuclei consisting of 2 protons and 2 neutrons (+2 charge)
- Can be stopped by sheet of paper
Beta radiation:
- Composed of high-energy electrons that are the product of the decomposition of a neutron or proton
- Can be stopped by thin sheet of aluminum foil, lucite, or plastic
Gamma radiation:
- High-energy electromagnetic radiation
- Can go through concrete and lead
Unstable atoms decay until…
It finds a stable nuclear configuration by emitting radioactive particles
Biochemistry:
Study of chemical processed in living organisms
Function of carbohydrates:
To store and provide energy for the body
Monosaccharides:
- Simplest type of carbohydrate
- Contain carbon, hydrogen, and oxygen in a ratio of 1:2:1
2 types of monosaccharides:
- Glucose and fructose
- Both are a six-carbon sugar called a hexose
Disaccharides
Consists of 2 monosaccharides joined together
2 types of disaccharides:
Sucrose (glucose + fructose)
Lactose (glucose + galactose)
Oligosaccharides:
3-6 monosaccharides joined together
Polysaccharides:
More than 6 and up to thousands of monosaccharides joined together-> called a starch
2 common polysaccharides:
Cellulose (made by plants)
Glycogen (made by animals)
Glycolysis:
Chemical pathway in the body that metabolizes glucose
Net result of glycolysis:
2 pyruvate
2 ATP
Anaerobic glycolysis:
Converts glucose to lactate instead of pyruvate as in aerobic glycolysis
Gluconeogenesis:
Process where the liver makes glucose from proteins and fats
Amino acids:
Composed of a carbon atom bonded with four other groups: amine, carboxyl, hydrogen, and an R group
Dipeptide:
Union of 2 amino acids using a peptide bond
Peptides/polypeptides:
Groups of fewer than 30 amino acids joined together
Fatty acids:
Consist of a hydrocarbon chain with an acid group ( the carboxyl group) at one end
Triglycerides:
Neutral fat that is joined by 3 fatty acids joined to a glycerol/backbone structure
Phospholipids:
Consists of 2 fatty acid chains and a phosphate group
Cholesterol:
Composed of a 4-ring structure and a side chain
Function of fats:
- Insulates body organs against shock
- Maintain body temp
- Keep skin and hair healthy
- Promotes healthy cell function
- Energy stores
Phospholipid function:
Essential component of cell membrane
Cholesterol:
Precursor for many important biological molecules such as steroids
Natural lipids are classified as:
Unsaturated, polyunsaturated, and saturated
Saturated fats:
No double bonds between carbon atoms of the fatty acid chains
Unsaturated fats:
One or more double bonds between carbon atoms of the fatty acids chains
Nucleic acids are found:
In all living cells and viruses
DNA structure:
Composed of deoxyribose and a phosphate
Amphoretic:
..
Pentose:
5 carbon sugar
Ribose:
5 carbon carbohydrate
