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Definition
| Anything that takes up space and has mass. |
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| A substance that cannot be broken down further to other substances by chemical reactions. |
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| A substance consisting of two or more different elements in a fixed ratio. |
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| The 25 percent of natural elements required for an organism to live a healthy life. |
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| Number of elements that occur naturally |
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Definition
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| The elements that make up ___ of living matter. |
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Definition
| Oxygen, carbon, hydrogen and nitrogen; 96% |
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| The remaining 4% of elements that make up an organism's mass, required in only minute quantities. |
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Definition
| The smallest unit of matter that still retains the properties of an element. |
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| The three subatomic particles |
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Definition
| Neutrons, protons, electrons. |
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Definition
| The dense core at the center of an atom composed of densely packed protons and neutrons. |
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Definition
| The unit of measurement for subatomic particles, roughly equivalent to the weight of one proton or one neutron and the AMU. |
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Definition
| The number of protons that is unique to that element, written as a as a subscript to the left. It never changes. |
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| How to calculate the number of electrons. |
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Definition
| If an atom is neutral, given that electrons occur in the same number of protons, you simply take the atomic number. |
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Definition
| The number of protons and neutrons combined, written as a superscript to the left. |
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Term
| How to calculate the number of neutrons |
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Definition
Mass number - atomic number
or
Superscript - subscript |
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Definition
| Total mass of the atom, roughly estimated by the number of protons and neutrons in Daltons. |
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Term
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Definition
| Atoms of the same element with a different number of neutrons. |
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Term
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Definition
| An unstable atom of an element with a different number of neutrons that decays spontaneously by giving off particles and energy, which can create an atom of a different element |
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Definition
| The energy of an object in relation to its location or structure. |
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Term
| How is potential energy from structure different from potential energy from location. |
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Definition
| Both have a tendency to go from high unstable energy to low, stable energy levels, but location-based potential energy can be expended all at once where as structural potential energy is expended in increments as the electrons that were resisting the pull of the protons goes from electron shell to electron shell, like a ball on a staircase. |
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Term
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Definition
| Concentric circles on which electrons are found at different distances from the nucleus, each denoting their own energy level and fixed number of spots for electrons. |
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Definition
| The outermost electrons in the valence shell. |
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Term
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Definition
| The outermost electron shell upon which the chemical behavior of an element is largely dependent. |
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Definition
| The three dimensional space where an electron is found 90% of the time. |
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Definition
| The attractions that hold together atoms. |
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Definition
| The sharing of a pair of valence electrons by two atoms. |
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Definition
| Two atoms held together by a covalent bond. |
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Definition
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Definition
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Definition
| Single pair of shared electrons |
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Definition
| Two pairs of shared electrons |
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Term
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Definition
| The bonding capacity of an atom, equal to the number of unpaired electrons required to complete the atom's valence shell. |
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Definition
| The attraction of a particular atom for the electrons of a covalent bond. |
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Definition
| When electrons are shared equally between two atoms due to equal electronegativity, and the tug-of-war attraction becomes a stand off, usually between two atoms of the same element. |
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Term
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Definition
| When one atom is bonded to an atom with a different electronegativity and the electrons are not shared equally. |
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Term
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Definition
| When the electronegativity between two atoms is so different that a bond is formed through the theft of an electron from one atom in the bond. |
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Definition
| An atom that has lost or gained an electron through an ionic bond, thus becoming charged. |
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Definition
| A positively charged ion due to the loss of an electron in an ionic bond. |
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Definition
| A negatively charged ion due to the gain of an electron in an ionic bond. |
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Definition
| Compounds formed by ionic bonds with crystalline lattice-like structures. |
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Definition
Another word for salt, which, unlike covalent bonds, does not indicate the size and number in its formula, but only the ratio of elements to one another in its structure.
NaCl is a ratio, not a specific molecule. |
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Definition
| The noncovalent attraction between the positively charged hydrogen and an electronegative atom. |
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Term
| Val der Waals Interactions |
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Definition
| Weak bonds between all atoms due to the ever changing asymmetrical accumulation or loss of electrons in an atom's electron shells that creates attraction between atoms. |
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Term
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Definition
| The making and breaking of chemical bonds, leading to changes in the composition of matter. |
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Definition
| The starting materials in a chemical reaction. |
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Definition
| The ending materials in a chemical reaction. |
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Term
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Definition
| The point at which the reactions converting reactant to products or products to reactants offset one another as they occur at the same time. This does not mean that the concentrations of reactants and products are equal, but only that they have stabilized at a particular ratio. |
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Term
| How the periods on the Periodic Table are arranged |
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Definition
| So that each period contains the same number of orbitals. |
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Term
| The far right column/group/family of the periodic table |
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Definition
| is the noble gases, which are inert, due to having full valence shells. |
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