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| Anything that has mass and occupies space |
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| The study of the composition of matter and the changes that matter undergoes |
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| a logical, systematic approach to the solution of a scientific problem |
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| What are the 4 states of matter? |
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| Solid, liquid, gas, and plasma |
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| matter with a definite shape and volume |
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| Matter with an indefinite shape, but a definite volume |
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| Matter with an indefinite shape and volume |
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| A measure of the amount of matter an object contains |
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| A measure of the space occupied by an object |
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| A property that depends on the amount of matter in a sample |
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| A property that depends on the type of matter in a sample |
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| Matter that has a uniform and definite composition |
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| A quality or condition of a substance that can be observed or measured without changing the substance's composition |
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| The gaseous state of a substance that is generally a liquid or solid at room temperature |
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| A change where some properties of a material change, but the composition of the material does not. |
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| A physical blend of two or more components |
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| A mixture in which the composition is not uniform throughout |
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| (or solution) a mixture in which the composition is uniform throughout |
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| Any part of a sample with uniform composition and properties |
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| The process that separates a solid from a liquid |
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| A process that separates two liquids |
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| The simplest form of matter that has a unique set of properties |
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| A substance that contains two or more elements chemically combined in a fixed proportion |
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| A change that produces matter with a different composition than the original matter |
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| The ability of a substance to undergo a specific chemical change |
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| A substance present at the start of a chemical reaction |
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| A substance produced in a chemical reaction |
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| A solid that forms and settles out of a liquid mixture |
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| The law of conservation of mass |
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| States that in any physical change or chemical reaction, mass is neither created nor destroyed |
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| A quantity that has both a number and a unit |
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| A given number is written as the product of two numbers: a coefficient and 10 raised to a power |
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| A measure of how close a measurement comes to the actual or true value of whatever is being measured |
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| A measure of how close a series of measurements are to one another |
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| The correct value based on reliable references |
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| The value measured in a lab |
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| the difference between the experimental value and the accepted value |
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| experimental value - accepted value |
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| All of the digits that are known in a measurement, plus a last digit that is estimated |
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| What happens to the density of a substance as its temperature increases? |
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| The smallest particle of an element that retains its identity in a chemical reaction |
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1. All elements are composed of tiny indivisible particles called atoms.
2. Atoms of the same element are identical. The atoms of any one element are different from those of any other element.
3. Atoms of different elements can physically mix together or can chemically combine in simple whole-number ratios to form compounds.
4. Chemical reactions occur when atoms are separated, joined, or rearranged. Atoms of one element, however, are never changed into atoms of another element as a result of a chemical reaction. |
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| Negatively charged subatomic particles located outside the nucleus |
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| Neutrally charged subatomic particles located inside the nucleus |
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| Positively charged subatomic particles located inside the nucleus |
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| Through a study of alchemy, Rutherford proposed that the atom is mostly empty space. He concluded that all the positive charge and almost all the mass are concentrated in a small region that has a positive charge, which he called the nucleus. |
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| In this atom, the protons and neutrons are located in the nucleus. The electrons are distributed around the nucleus and occupy almost all the volume of the atom. |
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| Atomic number is equal to... |
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| ...the number of protons (and number of electrons) |
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| The total number of protons and neutrons in an atom |
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| Atoms that have the same number of protons but different numbers of neutrons |
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| The weighted average mass of the atoms in a naturally occurring sample of an element |
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| Atomic mass (formula) based on relative abundance |
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| (mass of isotope 1)+(percent abundance/100) x (mass of isotope 2) + (percent abundance/100) etc. |
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| Each horizontal row of the periodic table |
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| (or family) each vertical column of the periodic table. Elements within a group have similar chemical and physical properties |
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| The problem with Rutherford's atomic model |
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| It could not explain the chemical properties of elements. :( |
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| in this model, an electron is found only in specific circular paths, or orbits, around the nucleus. |
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| The fixed energies an electron can have |
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| A quantum of energy is the amount of energy required to move an electron from one energy level to another |
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| The modern description of an atom, discovered by Erwin Schrödinger. It determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus. |
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| A region of space in which there is a high probability of finding an electron |
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| Electrons occupy the orbitals of the lowest energy first |
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| Pauli Exclusion Principle |
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| An atomic orbital may describe at most two electrons |
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| Electrons occupy orbitals of the same energy in a way that makes the number of electrons with the same spin direction as large as possible |
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| The wave's height from zero to the crest |
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| Represented by the Greek letter lambda, is the distance between the crests of a wave |
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| Represented by the Greek letter nu, is the number of wave cycles to pass a given point per unit of time |
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| The lowest possible energy of an electron |
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| When elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties |
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| Good conductors, high luster, solids at room temperature (except mercury), ductile, malleable |
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| poor conductors, brittle when solid, mostly gas |
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| The nonmetals of group 7A |
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| Group B elements. Atoms where the highest occupied S sublevel and a nearby D sublevel contain electrons. |
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| (lower B section) the highest occupied S sublevel and a nearby F sublevel contain electrons |
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| One half of the distance between the nuclei of two atoms of the same element when the atoms are joined |
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| Increases down group, decreases across period |
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| An atom with a positive or negative charge |
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| An ion with a positive charge. Always smaller than the atoms from which they form. |
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| An ion with a negative charge. Always larger than the atoms from which they form. |
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| The energy required to remove an electron from an atom |
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| Decreases down group, increases across period |
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| Increases down group, decreases across period |
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| The ability of an atom of an element to attract electrons when the atom is in a compound |
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| Decreases down a group, increases across a period |
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| The electrons in the highest occupied energy level of an atom |
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| In forming compounds, atoms tend to achieve the electron configuration of a noble gas |
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| Compounds composed of cations and anions. Usually composed of metal cations and nonmetal anions. Generally have a high melting point. Usually are crystaline solids at room temp. |
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| Diagrams that show valence electrons as dots |
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| The electrostatic forces that hold ions together in ionic compounds |
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| A neutral group of atoms joined together by covalent bonds |
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| Formed when one pair of electrons is shared |
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| Formed when two pairs of electrons are shared |
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| Formed when two pairs of electrons are shared |
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| A molecule that consists of two atoms |
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