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Chemistry Chapter 4
WOOT
23
Chemistry
11th Grade
12/13/2010

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Term
which type of solid materials are typically hard, have high melting points, and poor electrical conductivities (2)
Definition
ionic and covalent
Term
what is a correct description of metallic bonding? (ions to electrons)
Definition
positively charged metal ions are attracted to delocalized electrons
Term
Explain which has a bigger boiling point: CH3COOH or C2H5OH? (4)
Definition
CH3COOH has the biggest boiling point because, although they both have hydrogen bonds, CH3COOH has a bigger mass, so its bonds are harder to break;
more electrons, stronger van der Walls;
boiling point is based on intermolecular forces;
Term
Describe the metallic bonding present in aluminum and explain why aluminum has a higher melting point than sodium. (3)
Definition
Metallic bonding in aluminum is between delocalized electrons and positive nucleus. Its melting point is higher than Na because it has a higher mass; more electrons; stronger van der Waals; bonds harder to break.
Term
Predict and explain which of the following compounds consist of molecules:
NaCl, BF3, CaCl2, N2O, P4O6, FeS, CBr4(2)
Definition
NaCl and CaCl2 are the only compounds that are not compounds;
they have high differences in electronegativity, >1.8
Term
State the structures of and the bonding in diamond and graphite. (2)
Definition
Diamond has carbon bonds that are tetrahedrally arranged , with a 109.5 bond angle.
Graphite has carbon bonds that are held by van der Waals in parallel layers of trigonal bonding.
Term
Compare and explain the hardness and electrical conductivity of diamond and graphite. (4)
Definition
Diamond is a poor conductor, because it has no delocalized electrons;
It is extremely hard because it has a rigid structure;
Graphite is a good conductor because it has delocalized electrons;
It is soft because it has layers that can slide.
Term
Predict and explain how the hardness and electrical conductivity of C60 fullerene would compare with that of diamond and graphite. (4)
Definition
Fullerene is softer than diamond, but harder than graphite because the molecules can move over each other;
It conducts better than diamond, but worse than graphite;
C60 has less delocalized electrons than graphite;
Term
outline the principles of the valence shell electron pair repulsion (VSEPR) theory. (3)
Definition
electron pairs in the outer shell of an atom repel each other and position themselves as far away as possible;
negative charge centers thus determine shape of molecule (double, triple, single bonds all count as one center);
lone pairs of electrons repel the most and cause the most distortion of shape;
Term
Define ionic bond.
Definition
Electrostatic attraction between oppositely charged ions
Term
define covalent bond.
Definition
electrostatic attraction between a pair of electrons and positively charged nuclei
Term
As bond length increases, bond strength...
Definition
decreases.
Term
Put the three intermolecular forces in order of strength
Definition
van der Waals, dipole-dipole, hydrogen bond
Term
Describe the metallic bond.
Definition
electrostatic attraction between a lattice of positive ions and delocalized electrons.
Term
Name two physical properties associated with metals.
Definition
malleability, and ductility
Term
Bond angle of trigonal
Definition
120
Term
bond angle of pyramidal
Definition
107
Term
bond angle of tetrahedral
Definition
109.5
Term
bond angle of "bent" (only one lone pair)
Definition
117
Term
bond angle of "bent" (two lone pairs)
Definition
105
Term
Explain the expression "like dissolves like."
Definition
Ionic compounds are soluble in polar solvents
covalent compounds are soluble in non-polar solvents
Term
Ionic compounds have ______ structures.
Definition
lattice
Term
What is a dative bond?
Definition
a bond where one atom shares both electrons
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