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51 Cards in this Set
- Front
- Back
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element
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a substance that cannot be broken down to other substances by chemical reactions
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compound
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a substance consisting of two or more different elements combined in a fixed ratio
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4 major naturally occurring elements in the human body
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O, C, H, N
Oxygen, Carbon, Hydrogen, Nitrogen |
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atomic number
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the number of protons, unique to that element
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mass number
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the sum of the protons plus neutrons in the nucleus of an atom
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trace elements
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elements required by an organism in only minute quantities
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atom
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the smallest unit of matter that still retains the properties of an element
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dalton
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unit of measurement = atomic mass unit (amu)
roughly 1 proton or neutron |
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atomic mass
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approximation of the total mass of an atom
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isotopes
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atomic forms that have the same number of protons, but different numbers of neutrons, therefore having greater mass
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radioactive isotope
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one in which the nucleus decays spontaneously, giving off particles and energy
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energy
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the capacity to cause change, for instance by doing work
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potential energy
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energy based on postition, location, or structure
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energy levels
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different states of PE that electrons have in an atom, based on electron shells
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valence electrons
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outermost electrons
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valence shell
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outermost electron shell
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orbital
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the 3-dimensional space where an electron is found 90% of the time
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chemical bonds
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attraction bet. two atoms, based on sharing electrons or positive and negative charges
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covalent bond
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the sharing of a pair of valence electrons by two atoms
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molecule
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two or more atoms held together by covalent bonds
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single bond
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a pair of shared electrons
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single bond
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a pair of shared electrons
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double bond
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two pairs of valence electrons are shared between two atoms
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structural formula
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ex. H - H
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molecular formula
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ex. H subscript 2
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electronegativity
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an atom's attraction for electrons in a covalent bond
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valence
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bonding capacity of an atom
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nonpolar covalent bond
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electrons are shared equally
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polar covalent bond
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unequal sharing of electrons
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ion
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a charged atom or molecule
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double bond
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two pairs of valence electrons are shared between two atoms
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cation
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positively charged ion
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structural formula
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ex. H - H
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molecular formula
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ex. H subscript 2
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electronegativity
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an atom's attraction for electrons in a covalent bond
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valence
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bonding capacity of an atom
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nonpolar covalent bond
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electrons are shared equally
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polar covalent bond
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unequal sharing of electrons
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ion
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a charged atom or molecule
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cation
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positively charged ion
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anion
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a negatively charged ion
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ionic bond
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attraction between anion and cation because of opposite charges
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ionic compounds
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(salts) compounds formed by ionic bonds, ex. NaCl (sodium chloride)
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weak chemical bonds
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ionic bond, hydrogen bond
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hydrogen bond
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formed when a hydrogen atom covalently bonded to one electronegative atom is also attracted to another electronegative atom
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van der Waals intereactions
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weak attractions between molecules or parts of molecules that are brought about by localized charge fluctuations
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chemical reactions
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the making and breaking of chemical bonds, leading to changes in the composition of matter
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reactant
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starting materials in a chemical reaction
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product
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ending result in a chemical reaction
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chemical equilibrium
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the point at which the reactions offset one another exactly
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T/F All chemical reactions reversible.
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T
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