Chemistry First Semester Final Exam Vocabulary

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Mass

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a measure that reflects the amount of matter.

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weight

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a measure of an amount of matter and also the effect of Earth's gravitational pull on that matter.

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metric units

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a decimal measurement of the metric system.

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SI units

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a system of physical units

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density

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the amount of mass per unit volume.

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scientific notation

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expresses any number as a number between 1 and 10 (known as a coefficient) multiplied by 10 raised to a power (known as an exponent).

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accuracy

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refers to how close a measured value is to an accepted value.

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precision

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refers to how close a series of measurements are to one another.

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states of matter

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the physical forms in which all matter naturally exists on Earth - most commonly as a solid, liquid or a gas.

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properties of matter

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skip for now

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substances

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matter that has definite composition; also known as a chemical.

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mixtures

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a physical blend of two or more pure substances in any proportion in which each substance retains its individual properties.

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element

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a pure substance that cannot be broken down into simpler substances by physical or chemical means.

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compound

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a chemical combination of two or more different elements.

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heterogeneous mixture

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a mixture that does not have a uniform composition and in which the individual substances remain distinct.

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homogeneous mixture

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a mixture that has a uniform composition throughout and always has a single phase; also called a solution.

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solution

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a uniform mixture that can contain solids, liquids or gases; also called a homogeneous mixture.

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physical properties

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a characteristic of matter that can be observed or measured without changing the samples composition.

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chemical properties

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the ability or inability of a substance to combine with or change into one or more new substances.

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physical changes

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a type of change that alters the physical properties of a substance but does not change its composition.

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chemical changes

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a process involving one or more substances changing into new substances.

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law of conservation of mass

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states that mass is neither created or destroyed during a chemical reaction but is conserved.

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Dalton' atomic theory

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states that matter is composed of extremely small particles called atoms.

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atom

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the smallest particle of an element that retains all the properties of that element.

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electron

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a negatively charged, fast moving particle with an extremely small mass that is found in all forms of matter and moves through the empty space surrounding an atom's nucleus.

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proton

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a subatomic particle in atom's nucleus that has a positive charge of 1+.

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neutron

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a neutral, subatomic particle in atom's nucleus that has a mass nearly equal to that of a proton.

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nucleus

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the extremely small, positively charged, dense center of an atom that contains positively charged protons and neutrons.

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Rutherford's experiment and discovery

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he discovered the nucleus

**Come back to later???***

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JJ Thompson's discovery

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he made a model of an atom called the plum pudding model.

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atomic number

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the number of protons in an atom.

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mass number

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the number after an elements name representing the sum of it's protons and neutrons.

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calculating the number of protons

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is it's atomic number.

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calculating the number of neutrons

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mass number - atomic number.

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calculating the number of electrons

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same as the number of protons.

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calculating the mass number

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numbers of protons + number of neutrons

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isotopes

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atoms of the same element with different numbers of neutrons.

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calculating average atomic mass

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the weighted average mass of the isotopes of that element.

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electromagnetic radiation

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a form of energy that exhibits wavelike behavior as it travels through space.

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electromagnetic spectrum

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includes all form electromagnetic radiation, with the only differences in the types of radiation being their frequencies and wavelengths.

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wavelength

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the shortest distance between equivalent points on a continuous wave.

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frequency

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the number of waves that passes a given point per second.

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amplitude

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the wave's height from the origin to a crest.

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speed of light

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186,282 miles per second

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calculating wavelength

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wavelength = c / v

v=frequency
c=known constant

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calculating frequency

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v = c / wavelength

v = velocity
c = known constant

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atomic emission spectrum

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a set of frequencies of electromagnetic waves give off by atoms of an element.

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ground state

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the lowest allowable energy state of an atom.

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excited state

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a higher than normal energy level than an atom's ground state

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quantum mechanical model

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an atom model in which electrons are treated as waves.

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atomic orbitals

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a three-dimensional region around the nucleus of an atom that describes an electron's probable location.

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principle quantum number

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assigned by the quantum mechanical model to indicate the relative sizes and energies of atom orbitals.

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sublevels

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Come back to this one.

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electron configurations

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the arrangement of electrons in an atom.

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Pauli exclusion principle

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a maximum of two electrons can occupy a single atomic orbital but only if the electrons have opposite spins.

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Hund's rule

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single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins can occupy the same orbitals.

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Aufbau principle

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each electron occupies the lowest energy orbital available.

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noble gas configurations

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An electron structure of an atom or ion in which the outer electron shell contains eight electrons, corresponding to the electron configuration of a noble gas, such as neon or argon.

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valence electrons

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the electrons in atom's outermost orbitals.

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Mendeleev

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discovered twelve elements and developed the periodic table.

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Moseley

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discovered that atoms of each element contain a unique number of protons in their nuclei

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periodic law

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there is period repetition of chemical and physical properties of the elements when they are arranged by increasing atomic number.

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groups

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the boxes are arranged in order of increasing atomic number into a series of columns

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periods

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the rows on the periodic table

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representative elements

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groups I and II on the periodic table.

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transition elements

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groups III thru XII on the periodic table.

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metals

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elements that are generally shiny when smooth and clean, solid at room temperature, and good conductors of heat and electricity.

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alkali metals

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the group I elements (except for hydrogen).

any of the monovalent metals of group I.

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alkaline earth metals

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any of the divalent strongly basic metals of group II of the periodic table.

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transition metals

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an element in group III through XII that is contained in the D-block of the periodic table and, with some exceptions, is characterized by a filled outermost s orbital of energy level n, and filled or partially filled D-orbitals of energy level n1.

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inner transition metals

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a type of group b elements that is contained in the F-block of the periodic table and is characterized by a filled outermost orbital, and filled or partially filled 4f and 5f orbitals.

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lanthanide series

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in the periodic table, the F-block elements from period 6 that follow the element lanthanum.

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actinide series

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in the periodic table, the F-block elements from period 7 that follow the element actinium.

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nonmetals

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elements that are generally gases or dull, brittle solids that are poor conductors of heat and electricity.

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metalloids

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an element that has physical and chemical properties of both metals and nonmetals.

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Halogens

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a highly reactive group 17 element.

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noble gases

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an extremely unreactive group 18 element.

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valence electrons

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the electrons in an atom outermost orbitals.

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S-blocks

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the outermost energy level of an atom.

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P-blocks

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the second outermost energy level of an atom.

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D-blocks

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the third outermost energy level of an atom

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F-blocks

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the innermost energy level of an atom.

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transfer atomic radius

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ionization energy

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increases as you move left to right across a period and decreases in moving down a group.

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electronegativity

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indicates the relative ability of an element's atoms to attract electrons in a chemical bond.

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octet rule

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states that atoms lose, gain or share electrons in order acquire the stable electron configuration of a noble gas.

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chemical bond

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the force that holds two atoms together; may form by the attraction of a positive ion for a negative ion or by sharing electrons.

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cation

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an ion that has a positive charge.

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anion

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an ion that has a negative charge.

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polyatomic ions

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an ion made up of two or more atoms bonded together that acts as a single unit with a net charge.

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forming ions

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a positive ion forms when an atom loses one or more valence electrons in order to attain a noble gas configuration.

a negative ion forms with an atom gains valence electrons in order for attain a noble gas configuration.

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ionic bonds

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the electrostatic force that holds oppositely charged particles together in an ionic compound.

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writing / naming ionic formulas

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properties of ionic compounds

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physical structure - ions are packed into a regular repeating pattern that balances the forces of attraction and repulsion between the ions.

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crystal lattice

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a three-dimensional geometric arrangement of particles. Each positive ion is surrounded by negative ions and each negative ion is surrounded by positive ions.

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formula unit

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the simplest ratio of ions represented in an ionic compound.

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metallic bonds

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the attraction of a metallic cation for delocalized electrons.

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delocalized electrons

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the electrons involved in metallic binding that are free to move easily from one atom to the next throughout the metal and are not attached to a particular atom.

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properties of metals

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generally metals have moderately high melting points and high boiling points.

metals are malleable (can be hammered into sheets) and ductile (can be drawn into wire) and are generally durable.

metals are good conductors of heat and electricity.

transition metals have strong metallic bonds and are hard and strong. Alkali metals are considered soft.

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properties of alloys

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differ somewhat from the properties of the elements they contain.

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covalent / molecular bond

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a chemical bond that results from the sharing of valence electrons.

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molecule

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forms when two or more atoms covalently bond and is lower in potential energy than its constituent atoms.

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single bond

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also called sigma bonds, and occur when the pair of shared electrons is in an area centered between the two atoms.

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double bond

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a double covalent bond forms when two pairs of electrons are shared between two atoms.

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triple bond

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a triple covalent bond forms when three pairs of electrons are shared between two atoms.

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bond strength and length

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the strength of a covalent bond depends on the distance between the bonded nuclei.

the distance between the two bonded nuclei at the position of maximum attraction is called the bond length.

the shorter the bond length the stronger the bond.

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bond dissociation energy

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the amount of energy required to break a specific covalent bond.

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naming / writing molecular formulas

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naming acids

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structural formulas

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molecular model which uses letter symbols and bonds to show relative positions of atoms.

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Lewis dot (electron dot structure)

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VSEPR Theory

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Valence Shell Electron Pair Repulsion, based on an arrangement that minimizes d unshared pairs of electrons around the central atom.

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molecular shapes

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see table 8.6 on page 263

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polarity

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bond polarity

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depends on how strongly each of the bonded atoms attracts electrons.

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molecule polarity

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depends on the location and nature of the covalent bonds in the molecule.

polar molecules are attracted to an electric field, nonpolar molecules are not.

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solubility of polar molecules

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polar molecules are soluble, meaning they can dissolve in water.

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intermolecular forces

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in a covalent compound, the covalent bonds between atoms in molecules are strong but the attraction forces between molecules are relatively week.

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properties of covalent molecules

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alkanes

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hydrocarbons that contains only single bonds between atoms.

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names & formulas for the first ten alkanes

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See table 21.1 on page 751

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hydrocarbon

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simples organic compound composed only of the elements carbon and hydrogen.

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chemical reactions

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the process by which the atoms of one or more substances are rearranged to form different substances; occurrence can be indicated by changes in temperature, color, odor and physical state.

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reactants

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the starting substances in a chemical reaction

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products

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a substance formed during a chemical reaction.

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chemical equation

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a statement using chemical formulas to describe the identities and relative amounts of the reactants and products involved in a chemical reaction.

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coefficient

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in a chemical equation, the number written in front of a reactant or product

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balanced equation

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describes the lowest whole-number ratio of the amounts of all reactants and products

see table 9.2 on page 286 for steps for balancing equations

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symbols used in equations

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single-replacement reaction

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a chemical reaction that occurs when the atoms of one element replace the atoms of another element in a compound.

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activity series

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page 293-4??