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138 Cards in this Set
- Front
- Back
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Chemistry chpt. 1 |
The study of composition, structure, and properties of matter the process that matter undergoes. |
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Chemical chpt.1 |
Any substance that has defiant composition. |
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Mass chpt.1 |
Measure amount of matter. |
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Matter chpt. 1 |
Be defined as anything that has mass and takes up space. |
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Atom chpt. 1 |
Smallest unit of matter. |
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Element chpt. 1 |
Pure substance that can't be broken down and is made of one type of atom. |
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Compound chpt. 1 |
The substance that can be broken down and made from the atoms of two or more elements. |
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Extensive Properties chpt. 1 |
Depends on the amount of matter present. |
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Intensive Properties chpt. 1 |
Doesn't depend on the amount of matter present. |
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Physical Properties chpt. 1 |
A characteristic that can be observed or measured with out changing the identity of substance. |
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Physical Change chpt. 1 |
The change that doesn't involve the change of the identity of the substance. |
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Change of state chpt. 1 |
Physical change of substance on to another. |
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Solid chpt. 1 |
Definite volume and shape. |
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Liquid chpt. 1 |
Definite volume but not a definite shape. |
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Gas chpt. 1 |
Has neither definite volume or shape. |
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Plasma chpt. 1 |
High- temperature physically shape of matter, where atoms loose most electrons and particles that makeup atoms. |
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Chemical Properties chpt. 1 |
Substances ability to undergo changes that transforms into different substances. |
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Chemical change or reaction chpt. 1 |
The change of one or more substances that convert into different substances. |
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Reactants chpt. 1 |
The substances that react to chemical change. |
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Products chpt. 1 |
The substance snare formed by chemical change. |
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Mixture chpt. 1 |
A blend of two or more kinds of properties which retains its own identity and properties. |
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Homogeneous chpt. 1 |
Mixtures that uniform in composition. |
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Solution chpt. 1 |
Homogenous mixtures are called this. |
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Heterogeneous chpt. 1 |
Mixtures that are not uniform throughout. |
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Pure substance chpt. 1 |
Has a fixed composition. |
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Groups chpt. 1 |
Vertical column on the periodic table. |
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Family chpt. 1 |
Vertical column on the periodic table. |
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Periods chpt. 1 |
The horizontal column of elements in the periodic table. |
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Metal chpt. 1 |
The element that is a good conductor of heat and electricity. |
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Non-metal chpt. 1 |
The element that is a poor conductor of heat and electricity. |
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Metalloid chpt. 1 |
The element that has some characteristic of metals and non-metals. |
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Scientific Method chpt. 2 |
The logical approach to solving problems by observing, collecting data, formulating a hypothesis, testing hypothesis, and formulating theories that are supported by data. |
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System chpt. 2 |
Is a specific portion of matter in a given region of space that has been selected for study during an experiment or observation. |
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Hypothesis chpt. 2 |
A generalization about data to formulate or a testable statement. |
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Model chpt. 2 |
Science is more than a physical object; it is often an explanation of how phenomena occur and how data or events related. |
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Theory chpt. 2 |
A broad generalization that explains a body of facts or phenomena. |
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Quantity chpt. 2 |
Something that has a magnitude, size, or amount. |
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SI chpt. 2 |
A single measurement system. |
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Weight chpt. 2 |
Measure of gravitational pull on matter. |
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Derived Units chpt. 2 |
Combinations of SI base units. |
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Volume chpt. 2 |
Amount of space occupied by an object. |
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Density chpt. 2 |
A ratio mass to volume, mass divided by volume. |
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Accuracy chpt. 2 |
The closeness of measurements to the correct or accepted value of the quantity measured. |
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Precision chpt. 2 |
The closeness of a set of measurements of the same quantity made in the same way. |
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Precent Error chpt. 2 |
value experimental - value accepted value accepted x100 |
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Significant Figures chpt. 2 |
A measurement consist of all digits known with the certainty plus one final digit which is somewhat uncertain or is estimated. |
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Scientific Notation chpt. 2 |
The numbers where M is the number greater than or equal to but less than 10 and N is the whole number. ( mx10n) |
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Directly Proportional chpt. 2 |
Two quantities are two each other if dividing one by the other gives a constant value. |
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Inversely Proportional chpt. 2 |
The two quantities are to each other if their product is consistent. |
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Law of conservation of Matter chpt. 3 |
That mass has neither created nor destroyed during ordinary chemical reactions pr physical changes. |
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Law of definite proportions chpt. 3 |
Chemical compound contains the same elements in exactly the same proportions by mass regardless of the size of the sample or source of the compound is known. |
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Law of multiple proportions chpt. 3 |
Two or more different compounds are composed of the same two elements then the ratio of the masses of the second element is combined with a certain mass of the first element is always a ratio of small whole numbers. |
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Atom chpt. 3 |
The smallest particle of an element that retains the chemical properties of that element. |
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Nuclear Force chpt. 3 |
These short range proton - neutron, proton- proton, neutron-neutron forces hold the nuclear particles together. |
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Electron chpt. 3 |
Surrounding the nucleus is a region occupied by negatively charged particles. |
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Nucleus chpt. 3 |
Very small region located at the center of the atom. |
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Proton chpt. 3 |
The positive charged particles. |
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Neutron chpt. 3 |
The negative charged particles. |
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Atomic Number chpt.3 |
An element is the number protons of each atom of that element. |
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Isotope chpt.3 |
Atoms of the same elements that have different masses. |
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Mass Number chpt.3 |
The total number of protons and neutrons that make up the nucleus of a isotope. |
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Nuclide chpt.3 |
A general term for a specific isotope of an element. |
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Unified atomic mass unit |
is exactly 1/2 the mass of carbon 12 atom |
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Average atomic mass chpt.3 |
The weighted average of the atomic masses of the naturally occurring isotopes of an element. |
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Mole chpt.3 |
The amount of a substance that contains as many particles as there are atoms in exactly 12 g of carbon 12 |
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Avogadro's Number chpt.3 |
6.022141x10^23 is the number of particles in exactly one mole of pure substance. |
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Molar Mass chpt.3 |
The mass of one mole of a pure substance. |
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Electromagnetic Radiation chpt.4 |
Visible light which is a form of energy wavelike behavior as it travels through space. |
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Electromagnetic Spectrum chpt.4 |
All the forms of electromagnetic radiation from that. |
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Wavelength chpt.4 |
The distance between corresponding points on adjacent waves. |
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Frequency chpt.4 |
The number of waves that pass a given point in a specific time usually one second. |
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Photoelectric Effect chpt.4 |
Emission of electrons from a metal when light shines on a metal. |
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Quantum chpt.4 |
Energy is the minimum of energy that can be lost or gained by an atom. |
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Photon chpt.4 |
A particle of electromagnetic radiation having zero mass and carrying a quantum of energy. |
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Ground State chpt.4 |
Lowest energy state of an atom. |
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Excited State chpt.4 |
A atom has a high potential energy than it has in ground state. |
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Emission-line Spectrum chpt.4 |
4 beams of light were part of what is known as hydrogens. |
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Continuous Spectrum chpt.4 |
Observe the emission of a continuous range of fregancies of electromagnetic radiation. |
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Heisenberg Uncertainty Principle chpt.4 |
It is imposible to determine simuaneously both the position and the velocity of an electron
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Quantum Theory chpt.4 |
The mathematical wave properties of electrons and other very small particles. |
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Orbital chpt.4 |
3-Diminsonal region around the nucleus that indicates probable location of an electron. |
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Quantum Numbers chpt.4 |
Properties of atomic orbitals and properties of electrons in orbitals. |
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Principle of Quantum Numbers chpt.4 |
Symbolized by N, indicates the main energy level occupied by the electron. |
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Quantum Number/ angular Momentum |
Symbolized by L indicates the shape of the orbital. |
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Magnetic Quantum Number chpt.4 |
Symbolized by M indicates the orientation of an orbital around the nucleus. |
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Spin Quantum Number chpt.4 |
Has only two possible values-(+1/2-1/2)- which indicates the two fundamental spin states of an electron. |
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Electron Configuration chpt.4 |
Arrangement of electrons in an atom. |
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Aufbau Principle chpt.4 |
An electron occupies the lowest-energy orbital that can receive it. |
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Pauli Exclusion Principle chpt.4 |
No two electrons in the same atom can have the same set of four quantum numbers. |
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Hands Rule chpt.4 |
Orbitals of equal energy are each occupied by one electron, and all electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin state. |
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Noble Gas chpt.4 |
The group 18 on the periodic table. |
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Noble- gas configuration chpt.4 |
A outer main energy level occupied, in most cases by eight electrons. |
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Periodic Law chpt.5 |
The physical and chemical properties of the elements are periodic functions of their atomic number. |
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Periodic Table chpt.5 |
An arrangement of the elements in order of their atomic numbers so that elements with similar properties fell in the same column or group. |
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Lanthanides chpt.5 |
14 elements with atomic numbers from 58-71. |
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Actinides chpt.5 |
14 elements with the atomic numbers from90-103. |
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Alkali Metals chpt.5 |
The elements in group 1 of the periodic table. |
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Alkaline-earth Metals chpt.5 |
The elements in group 2 of the periodic table. |
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Transition Metals chpt.5 |
The d-block elements are metals with typical metallic properties. |
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Main-group elements chpt.5 |
The p-block elements together with the s-block elements. |
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Halogens chpt.5 |
The elements in group 17. |
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Atomic Radius chpt.5 |
May be defined as one-half the distance between the nuclei of identical atoms that are bonded together. |
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Ion chpt.5 |
Is an atom or group bounded atoms has a positive or negative charge. |
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Ionization Energy chpt.5 |
The energy required to remove one electron from a neutral atom of an element. |
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Electron Affinity chpt.5 |
The energy change that occurs when an electron is acquired by a neutral atom. |
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Cation chpt.5 |
The positive ion. |
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Anion chpt.5 |
The negative ion. |
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Valance Electrons chpt.5 |
A measure of the ability of an atom in a chemical compound to attract electrons from another atom in a compound. |
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Chemical Bond chpt.6 |
It is a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atom together. |
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Ionic Bonding chpt.6 |
Chemical bonding that results from the electrical attraction between cations and anions. |
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Covalent bonding chpt.6 |
The results from the sharing of electron pairs between two atoms. |
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Non-polar covalent bond chpt.6 |
A covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in a balanced distribution of electrical charge. |
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Polar chpt.6 |
They have an uneven distribution of charge. |
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Polar-covalent Bond chpt.6 |
Is a covalent bond in which the bonded atoms have an unequal attraction from the shared electrons. |
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Molecule chpt.6 |
A neutral group of atoms that are held together by the covalent bonds. |
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Molecular Compound chpt.6 |
A chemical compound whose simplest units are molecules. |
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Chemical Compound chpt.6 |
Indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts. |
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Molecular formula chpt.6 |
Shows the type and numbers of atoms combined in a single molecule of a molecular compound. |
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Bond energy chpt.6 |
Is the energy required to break a chemical bond and form neutral isolated atoms. |
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Electron-dot Notation chpt.6 |
Is an electron-configuation notation in which only valance electrons of an atom of a particular element are shown,indicated by dots placed around the elements symbol. |
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Lewis Structures chpt.6 |
Formulas in which atomic symbols are represent nuclei and inner-shell electrons, dot-pairs or dashes between two atomic symbols represent electron pairs in covalent bonds, and dot adjacent to only one atomic symbol represent unshared electrons. |
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Structural formula chpt.6 |
Indicates the kind,number,arrangement,a and bonds but not the unshared pairs of the atoms in a molecule. |
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Single Bond chpt.6 |
Is a covalent bond in which one pair of electrons shared between two atoms. |
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Multiple bonds chpt.6 |
Double and triple bonds |
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Resonance chpt.6 |
The bonding in molecules or ions that cannot be correctly represented by a single Lewis structure. |
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Ionic compound chpt.6 |
Is emptied of positive and negative ions that are combined so that the numbers of positive and negative charges are equal.
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Formula Unit chpt.6 |
The simplest collection of atoms from which an ionic compound's formula can be written. |
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Lattice Energy chpt.6 |
Is the energy released when one mole of an ionic crystalline compound is formed form the gaseous ions. |
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Polyatomic Ion chpt.6 |
A charged group of covalently bonded atoms. |
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Metallic Bonding\ chpt.6 |
The chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons. |
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Malleability |
Is the ability of a substance to be hammered or beaten into sheets. |
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Ductility chpt.6 |
The ability of a substance to be drawn,pulled,or extruded through a small opening to produce a wire. |
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VSEP Theory chpt.6 |
States that repulsion between the sets of valance electrons surrounding an atom causes these sets to be oriented as far as possible. |
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Hybridization chpt.6 |
Which is mixing of two or more atomic orbitals of similar energies on the same atom produce new hybrid atomic orbitals of equal energies. |
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Hybrid Orbitals chpt.6 |
Orbitals of equal energy produced by the combination of two or more orbitals of the same atom. |
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Dipole chpt.6 |
Created by equal but opposite charges that are separated by a short distance. |
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Hydrogen Bonding chpt.6 |
The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electrons of an electronegative atom in the nearby molecule. |
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London dispersion forces chpt.6 |
The intermolecular attractions resulting the constant motion of electrons and the certain of instantaneous dipoles. |
