Chemistry Qtr 1
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| The study of the nature of matter and the changes that matter undergoes | Chemistry
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| Anything that possesses mass and occupies space | Mass
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| What is the nature of matter? | The composition, the forces holding its parts together, and its observable properties
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| 4 Primary Classes of Compounds | Acids, Bases, Salts, Oxides
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| Law in which two or more elements combine in a fixed or definite proportion by mass | Law of Definite Proportions
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| Energy is neither created or destroyed | Law of Conservation of Energy
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| Matter is neither created or destroyed, just simply rearranged | Law of Conservation of Matter
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| Bond where there is a transfer of electrons, electrostatic bonding | Ionic Bonding
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| Bond where atoms share electrons | Covalent Bonding
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| Theory where same charges repel one another | Repulsive Theory
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| Does not cause a change in the chemical composition of a material (ex. melting, boiling, freezing) | Physical Change
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| Changes that result in the formation of new substances (ex. cremation, embalming) | Chemical Change
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| The ability to do work | Energy
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| The energy of motion (ex. H2O falling, a falling pen) | Kinetic Energy
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| Stored energy (ex. drawn bow, battery energy) | Potential Energy
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| The study of compounds usually containing elements other than carbon | Inorganic Chemistry
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| The study of certain carbon compounds | Organic Chemistry
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| The study of compounds produced by living organisms | Biochemistry
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| Compounds are.... | chemically united by bonds
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| Molecules that are not chemically united are in a.... | Solution
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| The study of those physical and chemical changes in the human body that are caused by the process of death | Thanatochemistry
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| The study of those types of matter and changes in matter related to the disinfection and preservation of a human remains | Embalming Chemistry
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| International System of Units is also known as... | The Metric System & SI Units
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| Standard unit of Length | meter (m)
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| Standard unit of Volume | liter (l)
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| Standard unit of Mass | kilogram (kg)
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| Standard unit of Heat | calorie (cal)
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| The 3 States of Matter | Solid, Liquid, Gas
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| A characteristic that can be observed without altering the chemical composition of a substance | Physical Property
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| Temperature at a given pressure at which a substance changes from the solid state to the liquid state | Melting Point
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| The same temperature as the melting point but the substance is changing from liquid to the solid state | Freezing Point
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| Temperature at a given pressure at which a substance changes from the liquid to the gaseous state | Boiling Point
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| Melting is a ________ ________ while the melting point is a _________ ________ | Physical Change; Physical Property
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| How much of something will dissolve in a given amount of water | Solubility
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| Expresses the relationship between its mass and volume | Density (mass/volume)
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| Ratio of the mass of the substance to the mass of an equal volume of water at the same temperature | Specific Gravity
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| A characteristic that can be observed when the substance is interacting with other forms of matter | Chemical Property
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| Whenever matter is burned in the presence of oxygen oxides are formed. This process is called.... | Combustion
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| Decomposition is initiated by.... | Hydrolysis
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| Process of water breaking apart is... | Hydrolysis
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| The state of matter is determined by... | the amount of energy it possesses
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| The most energetic state of matter is ______ The least energetic state of matter is _______ The state with an intermediate amount of energy is _______ | Gaseous State
Solid State
Liquid State
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| The state of matter where each particle possesses random rapid motion independent of the other particles | Gaseous State
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| The state of matter where the particles slide past one another | Liquid State
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| The state of matter where the particles vibrate around fixed positions | Solid State
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| A specific quantity of heat that is absorbed to convert 1 gram of a solid to 1 gram of the liquid at the substances melting point | Heat of Fusion
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| The amount of heat necessary to change 1 gram of a substance from the liquid to the gaseous state at the boiling point | Heat of Vaporization
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| The heat of fusion for water is _______ | 80 calories per gram
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| The heat of vaporization of water is ________ | 540 calories per gram
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| Any process that liberates heat is.... | Exothermic
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| Any process that absorbs heat is.... | Endothermic
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| Change in state directly from the solid state to the gaseous state | Sublimation
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| A measure of the amount of disorder or randomness | Entropy
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| Name the 3 states by highest entropy to least entropy | Gaseous, Liquid, Solid
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| 3 Properties of Gas | Compressibility, Expansivity, Diffusibility
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| The volume of a gas is equal to... | the volume of the container
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| Law which states that the volume occupied by a gas is inversely proportional to the pressure if the temp remains constant P1V1=P2V2 | Boyle's Law
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| Law which states that the volume of a fixed quantity of gas is directly proportional to its Kelvin temp if the pressure remains constant V1=V2 T1 T2 | Charles Law
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| Law that states as the temp of a gas increases the pressure increases and vice versa if the volume remains constant P1=P2 T1 T2 | Gay-Lussac's Law
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| Gases do not have a definite _____ or _______ | Shape; Volume
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| _____ do not have a constant shape but do have a definite _______ | Liquids; Volume
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| Solids have a definite ______ and _____ | Shape; Volume
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| Transition from liquid to gas that is a cooling process | Evaporation
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| Transition from gas to liquid | Condensation
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| When two opposing rates are equal | Equilibrium
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| The pressure exerted by a vapor when it is in equilibrium | Equilibrium Vapor Pressure
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| 2 Types of Matter | Pure substances & Mixtures
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| Substances that cannot be decomposed by further chemical means | Elements
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| Substances composed of two or more elements chemically united in a definite proportion by mass | Compound
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| Two or more nonchemically united substances that are in no definite proportion by mass | Mixture
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| The most abundant element on Earth is... | Oxygen
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| In the universe the most abundant element is... | Hydrogen
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| _______ mixtures are characterized by uniform properties throughout their contents; uniform composition | Homogeneous
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| _________ mixtures do not have uniform properties; not having uniform composition throughout | Heterogeneous
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| The smallest particle of an element | Atom
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| Atoms are composed of..... | A small dense positively charged nucleus, surrounded by negatively charged particles (electrons)
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| Name the 3 subatomic particles | Neutrons, Protons, Electrons
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| Where is the mass of an atom located? | Nucleus
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| Which subatomic particles are located in the nucleus? | Protons & Neutrons
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| Positively charged particle found in the nucleus of an atom, mass is 1 amu | Proton
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| The atomic number (z) is determined by.... | The number of protons, also the same number of electrons
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| Neutral subatomic unit found in the nucleus of an atom, mass is 1 amu | Neutron
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| Atoms are known to be.... | Neutral
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| Negatively charged particle found orbiting around the nucleus of an atom | Electron
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| The atomic mass number is.... | The total number of protons and neutrons
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| What is the force holding an atom together? | The interaction of the positively charged nucleus and the negative electrons
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| Atoms of the same atomic number and different masses | Isotopes
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| Isotopes have the same number of ______ & _______ but a different number of _________ | Protons & Electrons
Neutrons
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| Is it possible to tell the exact location of an electron? | No
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| The electrons in the outer most energy level | Valence Electrons
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| Valence electrons determine the..... | Chemical properties of the atom
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| Plots that estimate where electrons are found in energy levels | Orbitals
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| Each orbital can hold how many electrons? | 2
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| The s orbital holds a total of how many electrons? | 2
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| The p orbitals hold a total of how many electrons? | 6
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| A shorthand system used to symbolize the positions of electrons in atoms | Electron Configuration
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| The electron configuration give us 3 pieces of information... | 1) # of the energy level
2) Type of orbital
3) # of electrons in the orbital
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| Atoms that gain or lose an electron | Ions
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| If an atom loses one or more electron | Positive Ion
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| If an atom gains one or more electron | Negative Ion
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| Group IA | Alkali Metals
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| Group IIA | Alkaline Earth Metals
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| Group VIIA | Halogens
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| Group VIIIA | Noble Gases/Inert Gases
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| Rows on the periodic table are called.... | Periods
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| Elements to the left of the heavy line are... | Metals
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| Elements to the right of the heavy line are... | Non-Metals
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| Atoms that join together form... | Molecules
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| The smallest unit into which a compound may be divided and still retain the properties of that compound | Molecule
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| The net attractive interaction between two atoms in a molecule are... | Chemical Bonds
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| 2 Types of chemical bonds | Ionic and Covalent
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| Transfer of electrons from one atom to another results in... | Ionic Bond
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| The electrostatic attraction between a positive and negative ion | Ionic Bond
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| Bond formed by the sharing of electrons between two atoms | Covalent Bond
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| The sharing of one pair of electrons | Single Covalent Bond
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| The sharing of two pairs of electrons | Double Covalent Bond
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| The sharing of three pairs of electrons | Triple Covalent Bond
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| A measure of attractiveness of an atom for electrons | Electronegativity
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| Covalent bonds between unlike atoms | Polar Covalent Bonds
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| Covalent bonds between like atoms | Nonpolar Covalent Bonds
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