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Modules 1-7
Review flashcards for modules 1-7.
149
Chemistry
11th Grade
05/23/2013

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Term
Chemistry
Definition
The study of the composition of matter and the changes it undergoes.
Term
Organic Chemistry
Definition
Study of carbon compounds.
Term
Inorganic Chemistry
Definition
Study of compounds that do not contain carbon.
Term
Biochemistry
Definition
Study of processes that take place in organisms.
Term
Analytical Chemistry
Definition
Focuses on composition of matter.
Term
Physical Chemistry
Definition
Study of mechanism, rate, and energy changes in matter when undergoing change.
Term
Pure Chemistry
Definition
Pursuit of chemical knowledge for its own sake.
Ex: Study of metalloids and their properties.
Term
Applied Chemistry
Definition
Chemistry in use.
Ex: Use of metalloids in semiconductors for computer chips.
Term
Qualitative Data
Definition
Descriptions.
Ex: The solution is blue, the base feels slippery, or there are bubbles formed in the reaction.
Term
Quantitative Data
Definition
Measurements.
Ex: The test tube has a mass of 3.2 grams or the length of my shoe is 20 centimeters long.
Term
Scientific Method
Definition
1. State problem and collect data.
2. Formulate hypothesis.
3. Perform experiments.
Term
Independent Variable
Definition
The manipulated variable.
Term
Dependent Variable
Definition
The measured variable.
Term
Control
Definition
Remains unchanged in the experiment.
Term
Observations
Definition
Witnessed and can be recorded.
Term
Theories
Definition
Interpretations or explanations.
Term
Law
Definition
Summary of observed behavior.
Term
Matter
Definition
Anything that has mass and takes up space.
Term
Three states of matter
Definition
1. Solid
2. Liquid
3. Gas
Term
Solid
Definition
Particles packed tightly, usually dense, incompressable, and do not flow. Definite volume and definite shape.
Term
Liquid
Definition
Have a definite volume and the ability to flow. Do not have a definite shape. Takes shape of container it fills.
Term
Gas
Definition
Particles move rapidly and independently, fill the container they are in, and have the ability to flow. No definite shape or volume.
Term
Fixed Composition a.k.a. Pure Substance
Definition
Always has the same composition and internal properties. Can write a formula for it.
Ex: H2O, NaCl, C12H22O11, and N2
Term
Variable Composition a.k.a. Mixture
Definition
Cannot write a formula for it.
Term
Atoms
Definition
Smallest unit of matter.
Term
Elements
Definition
Same kind of atoms.
Ex: Carbon, oxygen, and hydrogen
Term
Compounds
Definition
Chemical combination of elements, forms molecules or crystals.
Term
Homogeneous
Definition
The same throughout the sample. All elements and compounds. If a mixture, it's called a solution.
Ex: Saltwater, sugar water, and air.
Term
Heterogeneous
Definition
Composition can vary within the sample. All mixtures that aren't solutions are heterogeneous.
Ex: Salad, pizza, soil.
Term
Physical Properties
Definition
Can be measured.
Ex: Size, shape, color.
Term
Physical Changes
Definition
Can be observed without changing the substance.
Ex: Melting, freezing, boiling.
Term
Chemical Properties
Definition
A description or characteristic of the substance that when observed causes the substance to be changed.
Ex: Flammable, corrosive, and reactivity.
Term
Chemical Changes
Definition
Composition of matter changes, a chemical reaction has occurred.
Ex: Decompose, rust, and burn.
Term
Other states of matter
Definition
Plasma and Bose Einstein Condensate (BEC)
Term
Plasma
Definition
Similar to gas, but some particles are ionized. Found in stars and neon lights.
Term
Bose Einstein Condensates (BEC)
Definition
At very low temperatures, atoms become blobs.
Term
Kinetic Molecular Theory (KMT)
Definition
Based on five assumptions:
1. Gases are made up of many tiny particles that are far apart.
2. The movement of the gas produce elastic explosions.
3. Gas particles possess kinetic energy because they are in constant motion.
4. There are no attraction or repulsion forces between particles.
5. The average kinetic energy is dependent upon the temperature.
Term
Six Properties of Gas
Definition
1. Expansion-Gases will fill their container.
2. Fluidity-Gases flow.
3. Low Density-Gases have low density.
4. Compressibility-Gases can be compressed into a smaller container.
5. Diffusion-Gases will completely mix in a container.
6. Effusion-Gases can be forced through a tiny opening.
Term
Heat
Definition
Total kinetic energy. Measured in joules(J).
Term
Temperature
Definition
Average kinetic energy. Measured in C or K. K=C+273
Term
Direction of Heat
Definition
Heat travels from warm to cold until equilibrium is met.
Term
Heat, temperature, and gases
Definition
As heat is added, temperature increases and the particles in the gas expand and move faster. Thus, the gas expands.
Term
What causes a phase change?
Definition
Change in temperature and pressure.
Term
Liquid to Gas
Definition
Vaporization-conversion of liquid to gas
Evaporation-conversion of liquid to gas at the surface and is not boiling, occurs in an open container
Term
Other Changes of State
Definition
Sublimation-solid directly to gas
Deposition-gas directly to solid
Term
Triple Point
Definition
Temperature and pressure at which all three phases can exist in equilibrium.
Term
Critical Point
Definition
The temperature and pressure at which the liquid and gas phase become indistinguishable.
Term
Proton
Definition
Mass: 1 amu
Charge: Positive
Symbol: p+
Location: Nucleus
Term
Electron
Definition
Mass: 0 amu
Charge: Negative
Symbol: e-
Location: Energy Levels
Term
Neutron
Definition
Mass: 1 amu
Charge: Neutral
Symbol: n0
Location: Nucleus
Term
Average Atomic Mass
Definition
[(Atomic Mass)(%Abundance)+(Atomic Mass)(%Abundance)]/100
Term
Facts about protons, electrons, and neutrons.
Definition
-Number of protons=atomic number
-Number of electrons=number of protons
-Number of neutrons=atomic mass- number of protons
Term
Isotopes
Definition
Same atomic number, but different atomic mass. Thus, there are a different number of neutrons than usual.
Term
Electromagnetic Spectrum (EM Spectrum)
Definition
Longest wavelength is the radio waves, then it is the microwaves, after that is infrared, next is visible light, then ultraviolet, after that is X rays, and the shortest wavelength is Gamma rays.
Term
Wave-Particle Nature of Light
Definition
Light travels as waves, but carries packets of energy called photons.
Term
Wavelength
Definition
Distance from the top of one wave to another.
Term
Frequency
Definition
How often the wave rises and falls at a specific point.
Term
Emission Spectrum
Definition
Spectrum of light released from excited atoms of an element.
Term
Endothermic
Definition
Absorbs/requires input of energy. Energy "enters" the system.
Term
Exothermic
Definition
Releases/emits/produces energy. Energy "exits" the system.
Term
Quantum Model
Definition
Probability of locating an electron at any place.
Term
Heisenberg Uncertainty Principle
Definition
It is impossible to know both the velocity and position of an electron at the same time.
Term
Principle Energy Level
Definition
Indicates main energy level occupied by e-. Always a whole number.
Term
Sublevels
Definition
Indicates shape or type of orbital.
Term
Orbitals
Definition
Each orbital holds a pair of electrons. Both electrons will spin in opposite directions.
Term
Electron Configurations
Definition
Shows the electron arrangement in an atom and always represents the lowest possible energies.
Term
Aufbau Principle
Definition
electrons fill orbitals that have the lowest energies first.
Term
Electron Configuration of Pb
Definition
1s2 2s2 2p6 3s2 3p6
Term
Shorthand Notation
Definition
Uses noble gases as a reference point.
Term
Orbital Notation
Definition
Uses lines to represent orbits and arrows to represent the spin of each electron.
Term
Hund's Rule
Definition
e- spread out within equivalent orbits.
Term
Radioactivity
Definition
Radiation is emitted during radioactive decay.
Term
Three Types of Radiation
Definition
1. Alpha Radiation
2. Beta Radiation
3. Gamma Radiation
Term
Alpha Particles
Definition
Helium nuclei emitted from a radioactive source. Consist of two protons and two neutrons which gives it a +2 charge.
Term
Beta Particles
Definition
Same properties as electrons.
Term
Gamma Ray
Definition
High energy photons emitted by radioactive isotopes. Most powerful form of radiation.
Term
Half Life
Definition
Time it takes for half of a radioactive isotope to decay.
Term
Nuclear Fission
Definition
Splitting of a nucleus into smaller parts. Initiated by hitting fissionable isotopes with neutrons. Only two fissionable isotopes are Uranium-235 and Plutonium-239.
Term
Nuclear Fusion
Definition
When nuclei combine to form a nucleus of greater mass.
Term
Nuclear Waste
Definition
Mainly, spent fuel rods from nuclear power plants. Made up of Uranium-235 and Plutonium-239.
Term
Period
Definition
Rows of periodic table. Currently, seven exist.
Term
Group
Definition
Columns of periodic table. Also called families. Have similar properties. Currently, there are eighteen.
Term
Alkali Metals
Definition
-Group 1
-Include all except H
-Soft metals
-Very reactive, not found in nature as free elements
-1 valence electron
Term
Alkaline Earth Metals
Definition
-Group 2
-Stronger, denser, and harder than Alkali metals
-Still too reactive to be found as free elements.
-2 valence electrons
Term
Transition Metals
Definition
-Groups 3-12
-Typical metals
-Less reactive
-Number of valence electrons vary
Term
P-Block Elements
Definition
-Groups 13-18
-Include metals, metalloids, and nonmetals
Term
Halogens
Definition
-Group 17
-Most active nonmetals
-React with metals to form salt
-7 valence electrons
Term
Metalloids
Definition
-Along zigzag line/ staircase
-Both metal and nonmetal properties
Term
Lanthanides
Definition
-Period 6
-Shiny metals
Term
Actinides
Definition
-Period 7
-All are radioactive
-No isotopes are known to be stable
Term
Valence Electrons
Definition
Outer most electrons that are available to be gained or lost. 8 valence electrons=chemically stable. Elements react to reach eight valence electrons.
Term
Ions
Definition
An atom or group of bonded atoms with a positive or negative charge.
Term
Positive Ions
Definition
Called cations. Form when an atom loses electrons.
Term
Negative Ions
Definition
Called anions. Form when an atom gains electrons.
Term
Atomic Radius
Definition
Half the distance between the nuclei of identical atoms that are bonded together. Size of the atom. Trend increases down and to the left.
Term
Ionization Energy
Definition
Energy required to remove one electron from a neutral atom. Trend increases up and to the right.
Term
Electronegativity
Definition
Measure of the ability of an atom in a chemical compound to attract electrons closer to it. Noble gases aren't included. Trend increases up and to the right.
Term
Metallic Activity
Definition
Trend increases down and to the left.
Term
Ionic Radii
Definition
Positive ions are smaller than an atom of the same element because they lose an electron. Negative ions are larger because they gain an electron.
Term
Ionic Bonds
Definition
-Transfer of electrons
-Metal and nonmetal
-Cation+anion
-Metals lose their valence e- and nonmetals gain a valence e-
Term
Lewis Dot Diagram
Definition
Visual interpretation of the number of valence electrons in an atom or ion.
Term
Properties of Ionic Bonding
Definition
-Hard, brittle, crystalline solids at room temp.
-High melting and boiling points
-Don't conduct as solids
-Do conduct when melted or dissolved in water
-Mot are soluble in water
-Called salts
Term
Metallic Bonding
Definition
-Cations in a sea of electrons
-Malleable-can be flattened
-Ductile-can be pulled into wire
-Bendable/shapeable
-Alloys-metal mixtures
Term
Chemical Formula
Definition
Show kinds and numbers of atoms in smallest representative unit.
Term
Oxidation Numbers
Definition
The charges that an atom takes on to obey the Octet Rule.
Term
Polyatomic Ion
Definition
Group of covalently bonded ions that have an overall charge.
Term
Properties of Molecular Compounds
Definition
-Formed when atoms share electrons
-Occurs between nonmetals
-Most have low melting points
-Not very conductive
-Soft
-Dissolve in water to form solution
Term
Single Bond
Definition
Share one pair of electrons. Group 17
Term
Double Bond
Definition
Share two pairs of electrons. Group 16
Term
Triple Bond
Definition
Share three pairs of electrons. Group 15
Term
Coordinate Covalent Bond
Definition
Shared pair of electrons in which both came from the same atom.
Term
Bond Dissociation Energy
Definition
Indicates the strength of a bond. The higher the energy, the stronger the bond.
Term
Mono-
Definition
1
Term
Di-
Definition
2
Term
Tri-
Definition
3
Term
Tetra-
Definition
4
Term
Penta-
Definition
5
Term
Hexa-
Definition
6
Term
Hepta-
Definition
7
Term
Octa-
Definition
8
Term
Nona-
Definition
9
Term
Deca-
Definition
10
Term
Valence Shell Electron-Pair Repulsion Theory
Definition
Valence electron pairs repel each other.
Term
Polar Bonds
Definition
Unequal sharing of electrons creates partially positive and partially negative ends. Called a dipole.
Term
Nonpolar Bonds
Definition
No partially charged regions are created resulting in equal sharing of electrons.
Term
Dispersion Forces
Definition
Occur between nonpolar forces. Weakest intermolecular forces.
Term
Dipole-Dipole Forces
Definition
Occur between polar molecules.
Term
Hydrogen Bonding
Definition
Occur between molecules with an H-F, H-O, H-N bond. Strongest form of intermolecular bonds.
Term
Mole
Definition
Defined as the number of carbon atoms in exactly twelve grams of carbon-12. Abbreviated mol. 1 mol=6.02x10^23. Used to measure matter. Used because atoms and molecules are too small to measure.
Term
Avogadro Number
Definition
6.02x10^23
Term
Percent Composition
Definition
Molar mass represents 100% of the mass one mole of a substance. Mass of each element compared to the total mass of the compound.
Term
Empirical Formulas
Definition
Lowest whole number ratio of elements. All ionic formulas are empirical.
Term
Subscripts
Definition
Tells how many atoms of a particular element are in a compound.
Term
Coefficients
Definition
Quantity of molecules in a compound.
Term
Synthesis
Definition
Two or more substances combine to form a new compound.
Term
Decompsition
Definition
A single compound undergoes a reaction that produces two or more simpler substances.
Term
Single Replacement
Definition
A+BX->AX+B
BX+Y->BY+X
Term
Double Replacement
Definition
The ions of two compounds exchange places in an aqueous solution to form two new compounds.
Term
Combustion
Definition
A substance combines with oxygen, releasing a large amount of energy in the form of light and heat.
Term
Mole-Mole Conversions
Definition
Given the number of moles of a substance to find how many moles of another substance are created from that in a chemical reaction.
Term
Mole-Mass Conversions
Definition
Given the number of moles of a substance to find how many grams of another substance are created from that in a chemical reaction.
Term
Mass-Mole Conversions
Definition
Given the mass of a substance to find how many moles of another substance are created from that in a chemical reaction.
Term
Mass-Mass Conversions
Definition
Given the mass of a substance to find how many grams of another substance are created from that in a chemical reaction.
Term
Mass-Volume Conversions
Definition
Given the mass of a substance to find how many liters of another substance are created from that in a chemical reaction.
Term
Mole-Particle Conversions
Definition
Given the number of moles of a substance to find how many particles of another substance are created from that in a chemical reaction.
Term
Limiting Reactant
Definition
Limits the amount of product that is produced.
Term
Excess Reactant
Definition
Reactant that produces more product than the limiting reactant. Does not affect how much product is created.
Term
Theoretical Yield
Definition
The amount of product expected to be recovered according to the limiting reactant.
Term
Actual Yield
Definition
The amount of product recovered in an actual experiment.
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