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92 Cards in this Set
- Front
- Back
- 3rd side (hint)
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Graphite and diamonds are both pure carbon. Why is graphite "soft" and "slippery" while diamonds are extremely hard?
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Graphite is 3 carbons bonded together. Diamond is 4.
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(T/F) The "need" individual atoms have for stability is the driving force for chemical bond formation.
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T
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(T/F) Chemical bonds involve mainly the valence electrons.
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T
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(T/F) Chemical stability is achieved by forming compounds with other atoms.
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T
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How does an atom with fewer than 8 electrons fill its valence level?
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It either looses or gains the electrons.
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Except for hydrogen and helium a filled outer electron layer contains _____ electrons.
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8
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How does compound formation fill the valence layers of the participating atoms?
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gain/loses, share
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What determines whether an atom loses or gains electrons or shares electrons during chemical bond formation?
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whichever is easier
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(T/F) The more electronegative atom can remove an electron from the less electronegative atom.
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T
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(T/F) Group 1A elements have very high electronegativities.
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F
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(T/F) Alkali and alkaline earth metals have high electronegativities.
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F
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(T/F) Halogens have 7 outer layer electrons and attract electrons strongly enough to take 1 more. Halogens have very high electronegativites.
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T
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(T/F) Because the outermost energy levels of the noble gases are filled, they neither give up or accept electrons.
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T
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(T/F) Neon has a higher electronegativity than sodium.
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F
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(T/F) Iodine has a higher electronegativity than fluorine.
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T
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(T/F) Because potassium and bromine are both in period 4, we can be certain that they have equivalent electronegativities.
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F
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(T/F) With the exception of the noble gases, the nonmetals have higher electronegativites than metals.
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T
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(T/F) Carbon possesses 4 valence electrons. Thus its electronegativity is neither strong nor weak, so carbon usually shares electrons when it chemically bonds to other atoms.
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T
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Bonds formed by the equal sharing of electrons are called _________ bonds.
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Covalent
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__________ bonds form when atoms of high electronegativity bond with atoms of low electronegativity.
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Ionic
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A particle that either a positive or a negative charge is called a(n) ___________.
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ion
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A negative ion is called a(n) _____________.
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anion
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A positive ion is called a(n) _________________.
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cation
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_____ bonds result from the attraction of cations and anions, i.e., oppositely charged ions.
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Ionic
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The ionic attraction between oppositely charged ions is called the ___________ _________.
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electrostatic force
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______ ______ ________ is a shortcut method to illustrate the bonding process.
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Lewis dot structures (electron dot notation)
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(T/F) In every ionic bond, the total of the negative charges on the anions must be equal to the total of the positive charges on the cations.
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T
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What is the structure of the compound resulting from the bonding of the Group 1 metal sodium and the Group 6 metal sulfur?
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Na₂S
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(T/F) In all cases of ionic bonding, highly electronegative nonmetals pull electrons away from weakly electronegative metals.
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T
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(T/F) Ionic bonding occurs whenever a nonmetal has enough attraction to pull away the valence electrons of a metal.
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T
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(T/F) Two atoms with similar electronegativities cannot bind ionically.
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T
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(T/F) Ionic bonds always unite elements from opposite sides of the Periodic Table.
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T
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(T/F) Atomic size gets smaller as you move across the Periodic Table from Group 1A to Group VIIA
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T
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(T/F) Atomic size gets larger as you move down a group from Period 2 to Period 6 elements.
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T
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(T/F) As atomic size decreases electrons are harder to remove.
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T
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(T/F) As atomic size decreases the ionization energy increases.
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T
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(T/F) Metals tend to lose electrons.
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T
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(T/F) Non-metals tend to gain electrons.
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T
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In ionic solids the regular and repeated three-dimensional pattern of arrangement of positive and negative ions is called the ____________ _________.
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Crystal Lattice
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(T/F) Individual ionic compounds don't normally exist.
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T
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The basic or simplest repeating unit of an ionic solid is called the ________ ____.
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Formula unit
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The formula unit for sodium chloride is ____________.
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NaCl
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(T/F) Pure water is a good conductor of electricity.
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F
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(T/F) Aqueous (i.e., water) solutions of ionic compounds conduct electricity because of the positively charged cations and negatively charged anions.
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T
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A chemical compound that ionizes when dissolved or melted to produce an electrically conductive medium is called a(n) _________.
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electrolyte
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What is a "weak electrolyte?"
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Poorly ionized and thus exhibit low conductivity
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(T/F) Covalent bonds are found in diatomic molecules such as O₂and polyatomic molecules such as H₂O.
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T
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(T/F) CH₄- methane - is a covalent compound.
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T
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The basic unit of a covalent compound is the _________.
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molecule
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____________ are separate, distinct particles formed by the bonding of a limited but specific number of atoms.
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molecules
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(T/F) Compared with ionic compounds, there is a weak attraction between molecules and molecules generally have higher melting points.
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T
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Name the two classes of covalent bonds and distinguish between them.
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Nonpolar - individual bonds between atoms of near identical electronegativities
Polar covalent bonds - bonds between atoms having an electronegativity difference greater than 0 and less than 1.67 The more polar bonds are partially ionic |
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(T/F) Oxygen has 6 valence electrons. It needs to share 2 pairs of electrons, creating 2 covalent bonds in O₂
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T
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Sharing of two pairs of electrons is called a _________ _________.
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double bond
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Nitrogen atoms share ______ pairs of electrons in forming a triple bond.
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3
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(T/F) Within group IIA the atom with the greatest atomic radius is also the atom with the highest electronegativity.
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F
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(T/F) Within Period 2 the atom with the highest atomic number has the lowest electronegativity.
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F
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(T/F) In all cases of ionic bonding, highely electronegative nonmetals pull electrons away from weakly electronegative metals.
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T
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(T/F) Covalent bonds are found in diatiomic molecules such as O₂and polyatomic molecules such as H₂O.
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T
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A negatively chaged ion
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Anion
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VOCAB
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The number of pairs of electrons shared between atoms forming a covalent bond.
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Bond order
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VOCAB
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A positively charged ion.
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Cation
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VOCAB
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The holding together of atoms by attraction generated by the sharing of electrons or the transfer of electrons from one to another.
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Chemical bond
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VOCAB
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A substance in which two or more different types of elements are chemically bonded together.
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Compound
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VOCAB
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The bond formed by the sharing of electrons.
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Covalent bond
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VOCAB
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A molecule made from covalent bonds. Diatomic oxygen, methane, etc.
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Covalent molecule
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VOCAB
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A regular and repeated three-dimensional pattern of arrangement of positive and negative ions.
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Crystal lattice
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VOCAB
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A molecule composed of two atoms of the same element.
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Diatomic molecule
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VOCAB
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A chemical bond formed by the sharing of two pairs of electrons.
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Double bond
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VOCAB
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A chemical compound that ionizes when dissolved or melted to produce an electrically conductive medium.
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Electrolyte
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VOCAB
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The relative ability of an atom to attract electrons in a chemical bond.
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Electronegativity
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VOCAB
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Ionic attraction
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Electrostatic force
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VOCAB
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An ionic bond
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Electrovalent bond
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VOCAB
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The basic or simplest repeating unit of an ionic solid.
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Formula unit
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VOCAB
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Thought to be the electron configuration in metals where ALL of the valence electrons are shared by ALL of the atoms.
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Free Electron theory
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VOCAB
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A particle that has either a positive or negative charge.
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Ion
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VOCAB
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Having the character of an ion.
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Ionic
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VOCAB
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The bond formed between atoms of high electronegativity with atoms of low electronegativity which involves the transfer of one or more electrons from one atom to another. Simply the electrostatic attraction between opposite charges.
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Ionic bond
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VOCAB
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Made of positive and negative ions.
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Ionic compounds
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VOCAB
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A shortcut method to illustrate the bonding process. Also called the electron dot notation.
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Lewis dot structure
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VOCAB
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Very large molecules, such as proteins, fats and starches.
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Macromolecule
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VOCAB
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In metals, positive nuclei are considered to be surrounded by a "sea" of electrons.
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Metallic bonds
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VOCAB
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A group of atoms held together by strong attractive forces.
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Molecule
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VOCAB
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A covalent bond with no separation of charge.
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Nonpolar bond
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VOCAB
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Atoms are most stable if they have a filled outer layer of electrons.
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Octet rule
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VOCAB
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Compounds that contain both carbon and hydrogen.
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Organic compound
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VOCAB
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A covalent bond with a partial separation of charge
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Polar bond
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VOCAB
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A molecule with positive and negative "poles"
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Polar molecule
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VOCAB
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Molecules composed of two or more different elements.
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Polyatomic molecules
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VOCAB
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Good conductors of electricity because they are highly ionized when dissolved in water.
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Strong electrolyte
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VOCAB
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A chemical bond formed by the sharing of three pairs of electrons.
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Triple bond
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VOCAB
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Poorly ionized when dissolved and thus exhibit low conductivity.
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Weak electrolyte
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VOCAB
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