Chemistry – First Semester Terms – Flashcards

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mass
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the measure of matter in an object
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matter
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anything that has mass and takes up space
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atom
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the smallest unit of an element that maintains the chemical identity of that element
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element
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a pure substance that cannot be broken down into simpler, stable substances
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compound
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a substance made up of atoms from two or more elements joined by chemical bonds
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physical property
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a characteristic that can be observed or measured without changing the identity of the substance
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physical change
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a change that does not involve the change in the identity of the substance
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chemical property
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substance's ability to undergo changes to transform it into different substances
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chemical change
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a change that turns a substance into an entirely different substance
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change of state
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a physical change of a substance from one state to another
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solid
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something that has a definite shape and a definite volume
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liquid
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something that has no definite shape but has a definite volume
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gas
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something that has neither a definite shape or volume
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pure substance
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a fixed composition that has exactly the same characteristic properties and has exactly the same composition
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mixture
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a blend of two or more kinds of matter that can either be homogeneous or heterogeneous
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homogeneous
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uniform in composition
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heterogeneous
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un-uniform in composition
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group
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a vertical column of elements in the periodic table (see family)
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family
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a vertical column of elements in the periodic table (see group)
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period
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a horizontal row of elements in the periodic table
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metal
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elements that are good conductors of heat and electricity
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nonmetal
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elements that are poor conductors of heat and electricity
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metalloid
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accuracy
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how close the value is to the true or accepted value
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precision
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how reproducible the same value is
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isotope
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an element that has the same number of protons but different number of neutrons
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mass number
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equal to the number of protons plus the number of electrons
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atomic mass unit
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a unit used for expressing masses in atoms or molecules
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mole
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a counting number for atoms
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Avogadro's number
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(6.0221 x 10(^23) atoms / 1 mole
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molar mass
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grams of element (an average) / mole
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ground state
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the lowest energy state of an atom or particle in its most stable state (neutral, no charge)
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excited state
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an atom or partial with a charge
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orbital
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holds electrons in shells
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electron configuration
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using numbers and letters, no indication of spin.
ex: 1s(^2), 2s(^2), ... etc
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Aufbau principle
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an electron occupies the lowest energy orbital that can receive it
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Pauli exclusion principle
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no more than two electrons in each drawer. when you have two electrons in the same drawer, they have to have different spins
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Hund's rule
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orbitals of equal energy are filled by placing a single electron in each orbital and then doubling up after that. when single electrons are placed in orbitals of equal energy, they must have the same spin state
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ion
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charged atoms
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ionization
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when atoms give up electrons (form cations)
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ionization energy
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the energy required to remove an electron from an atom
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electron affinity
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when atoms gain electrons (forms anions)
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cation
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a positive ion
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anion
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a negative ion
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valence electrons
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electrons that are available for bonding
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electronegativity
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measure of the ability of an atom to attract electrons from other atoms (there is no transfer of electrons! it's how badly an element wants an electron!)
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chemical bond
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ionic bonding
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metal to nonmental bonding (transferring)
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covalent bonding
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nonmental to nonmetal bonding (sharing)
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nonpolar covalent bonding
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molecule
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structure type for COVALENT bonds (this vs ionic compounds)
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polar covalent bonding
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molecular compound
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a chemical compound where the simplest units are molecules
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molecular formula
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a formula that shows the number of atoms in a molecule
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electron-dot notation
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way to show an element with its valence electrons
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Lewis structure
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way to show bonds between COVALENT bonding
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structural formula
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a formula that indicates the location of atoms, number of bonds, and location of bonds
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ionic compound
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structure type for IONIC bonds (this vs molecules)
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formula unit
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a ratio of atoms - for IONIC bonding
ex. NaCL, MgO, LiBr
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lattice energy
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the energy that holds the atoms together in an ionic compound
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metallic bonding
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metal to metal bonding
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