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31 Cards in this Set
- Front
- Back
- 3rd side (hint)
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Chemical bond
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The force of attraction between any two atoms in a compound.
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78
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Lewis symbol
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A way or representing valence electrons with dots around the product's symbol.
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79
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Ionic bond
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An electrostatic attractive force between ions resulting from electron transfer. Metals and nonmetals usually react to form ionic bonds.
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G-7, 85
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Covalent bond
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Bond consisting of a pair of electrons shared between two atoms.
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G-4
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Writing formulas of Ionic Compounds from the Identities of the Component Ions:
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The charge of the atom must be identify (usually by the group or family). The cations and anions must combine in such a way that the resulting formula units has a net charge of zero.
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85
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Mono-
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1
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90
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Di-
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2
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90
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Tri-
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3
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90
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Tetra-
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4
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90
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Penta-
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5
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90
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Hexa-
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6
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90
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Hepta-
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7
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90
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Octa-
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8
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90
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Nona-
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9
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90
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Deca-
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10
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90
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Writing Names of Ionic Compounds from the Formula of the Compound
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The name of the cations appears first, followed by the name of the anion. The positive ion has the name of the element, while the negative ion is named by using the stem of the name of the element joined to the suffix -ide. If the ion exist in only one common charged form there is no ambiguity between formula and name.
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86
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Writing Formulas of Ionic Compounds from the Name
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Predict the charge of monatomic ions and remember the charge and formula of polyatomic ions. The relative number of positive and negative ions in the unit must result in a net compound of zero charge.
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88
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Naming Covalent Compounds from formula
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1. The names of the element are written in the order in which they appear in the formula.
2. A prefix indicating the number of each kind of atom found in the unit is place before the name of the element. 3. If only one atom of a particular kind is present in the molecule, the prefix mono= is usually omitted from the first element. 4. The stem of the name of the last element is used with the suffix -ide. 5. The final vowel in a prefix is often dropped before a vowel in the stem name. |
90
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Molecules
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Compounds characterized by covalent bonding.
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89
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Writing Formulas of Covalent Compounds
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Common names must be from memory, while compounds names using Greek prefixes are easily converted to formulas.
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91
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Electronegativity
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A measure of the ability of an atom to attract electrons in a chemical bond.
Generally from left to right across a periodic table the elctronegativity increases. As one top to bottom on a group the electronegativity decreases. |
83
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polar
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Bonds which have unequal sharing of electrons between the two atoms involved in bonding.
Examples of household polar molecules include sugar (sucrose). Polar molecules are generally able to dissolve in water (H2O) due to the polar nature of water. Polar molecules have slightly positive and slightly negatively charged ends. |
109 and wikipedi.org
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nonpolar
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There is (almost) no polarity (unequal share of electrons) in the bonds or because of the symmetrical arrangement of polar bonds.
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109
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Chemical polarity
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The dipole intermolecular forces between the slightly positively-charged end of one molecule to the negative end of another or the same molecule. Molecular polarity is dependent on the difference in electronegativity between atoms in a compound and the asymmetry of the compound's structure.
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wikipedia.org
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dipole
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A separation of positive and negative charge. The simplest example of this is a pair of electric charges of equal magnitude but opposite sign, separated by some, usually small, distance.
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wikipedia.org
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Asymmetry
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is the absence of, or a violation of, a symmetry (balance).
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wikipedia.org
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molecular structure
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The three-dimensional arrangement of the atoms that constitute a molecule. There are six basic shape types for molecules; linear, trigonal planar (shape of pyramid), Angular, Tetrahedral, Trigonal pyramidal, and Angular (nonlinear, bent).
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Wikipedia
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Linear
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Atoms are connected in a straight line. The bond angles are set at 180°. A bond angle is very simply the geometric angle between two adjacent bonds. For example, carbon dioxide has a linear molecular shape.
2 Bonded Atoms, 0 Nonbonding electron pairs. |
wikipedia
p 107 |
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trigonal planar (shape of a pyramid)
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Are somewhat triangular and in one plane (meaning a flat surface). Consequently, the bond angles are set at 120°. An example of this is boron trifluoride.
Bonding atoms 3 Nonbonding electron pairs 0 |
wikipedia
p 107 |
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tetrahedral
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Almost literally means "four surfaces." This is when there are four bonds all on one central atom, with no extra unshared electron pairs. In accordance with the VSEPR (valence-shell electron pair repulsion theory), the bond angles between the electron bonds are 109.5°. An example of a tetrahedral molecule is methane (CH4).
Bonding atoms 4 Nonbonding electron pairs 0 |
wikipedia
p 107 |
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non-linear shape, also known as bent or angular
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One of the most unquestionably important molecules any chemist studies is water, or H2O. A water molecule has a non-linear shape because it has two pairs of bonded electrons and two unshared pairs. Like in the other arrangements, electrons must be spaced as far as possible. Therefore, the bond angles here are 104.5°.
Bonding atoms 2 Nonbonding electron pairs 2 |
wikipedia
p 107 |
