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BJ Chem Ch 6 Bonds
BJ Chem Ch 6 Chemical Bonds
Question | Answer |
---|---|
The rule where atoms maximize stability by attaining a full valence shell (generally 8 electrons) | octet |
Type of bond which shares electrons | covalent |
Type of bond where a transfer of electrons occurs and then an electrostatic attraction | ionic |
Type of bond where delocalized electrons move through a "sea" | metallic |
Bond formed with a metal and metal | metallic |
Bond formed with two nonmetals | covalent |
Bond formed with a metal and nonmetal | ionic |
Tendency of an object to form two localized regions of opposite character. | polarity |
Choose: A sodium atom will (lose/gain) one electron to become a cation. | lose |
Choose: A chlorine atom will (lose/gain) one electron to become an anion. | gain |
Chemists use which lower case letter to identify polarity | delta |
Measure of an atom's ability to attract electrons to itself in a chemical bond | electronegativity |
Most electronegative element | flourine |
Name of man who created an electronegativity scale. | Linus Pauling |
The bond type between sodium and chloride. | ionic |
The bond type between carbon and hydrogen | covalent |
The bond type between copper and zinc (which makes the alloy brass) | metallic |
H-H is an example of a homonuclear _______ molecule. | diatomic |
Electronegativity differences of over 1.7 units generally result in a ________ bond. | ionic |
If the element with a higher electronegativity is less than 2.2, then the bond is ________. | metallic |
If the higher electronegativity is 2.2 or greater, then the element with the lower electronegativity determines the bond type. If it is also 1.7 or greater, then the bond type is __________. | covalent |
Two dimensional diagrams that show the bonds between different atoms | Lewis structures |
In a Lewis structure a ________ represents two electrons. | dash |
The number of valence electrons for nonmetals (except hydrogen) can be predicted by the formula: valence e = group number - 10. So, flourine (group 17 or 7A) would have ____ valence electrons. | 7 |
(T or F) Hydrogen can be used as the central atom ina polyatomic molecule. | False |
Atoms with valence structures similar to Group __ atoms are more likely to be the central atom in a polyatomic molecule. | 14 |
The central atom in a molecule is generally the one with the most (paired/unpaired) electrons. | unpaired |
The type of forces which hold covalently bonded atoms together. | Electrostatic forces |
Which seven elements generally occur as diatomic, covalent molecules? | H,N,O,F,Cl,Br,I |
Ionic compounds are represented by ________ units and do not contain distinct molecules. | formula |
Formula unit for Mg and Br | MgBr2 |
elements or compounds covalently bonded into a continuous three-dimensional networks (like SiO2, diamond) are called ______ covalent substances | network |
The type of bond which forms weaker intermolecular forces between molecules. | covalent |
In their solid state, most ionic solids are (poor/good) conductors of electricity. | poor |
What atoms do to attain the low-energy stable electron configurations of the noble gases. | bond |
_____ bonds share electrons among many atoms. | metalic |
_____ compounds generally form solid crystalline substances with high melting points. | ionic |
____ compounds consist of crystal lattics | ionic |
_____ compounds tend to be gases, liquids, soft solids, or brittle and crumbly solids. | covalent |
Adjective meaning "many atoms" | polyatomic |
(T/F) There is no purely covalent bond. | False |
(T/F) There is no purely ionic bond. | True |
Chemical bonds between atoms involve the rearrangine of _____ to maximize stability | electrons |
Draw the Lewis structure for HCN. The N has __ nonbonding electrons. | two |
Draw the Lewis structure for ammonia, NH3. The N has __ nonbonding electrons. | two |
Draw the Lewis structure for H2S. The S has ___ nonbonding electrons. | four |