Chapter 6 Study guide Flashcards
(23 cards)
Define chemical bond.
a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together
As independent particles, most atoms have what kind of energy?
high potential energy
As atoms bond with each other, what happens to their energy and stability?
it will decrease the potential energy, it will make the atoms more stable
What are the electrons involved in forming a chemical bond called?
valence electrons
What are shared in a covalent bond?
Electrons
If atoms that share electrons have an unequal attraction for the electrons, what type of bond do they form?
polar covalent bond
When atoms share electrons, the electrical attraction of an atom for the shared electrons is called the atom’s what?
electronegativity
If given the percentage ionic character, be able to determine the type of bond for the compound. (pg 176)
- 0-0.3 EN=0= 0%
- 3-1.7 EN=0.3=5%-50%
- 7-3.3 EN=3.3=50%-100%
What is the first step in drawing the Lewis dot structure?
you find the total of valence electrons
What is the last step in drawing a Lewis dot structure?
you go back through and count the number of valence electrons to make sure they match the first step.
When a covalent bond forms, what happens to the energy of the atoms?
decreases the energy
How do forces of attraction in molecules of molecular compounds compared to ionic bonding?
molecular compound will have a weaker attraction than the ionic bonding
Compared with energies of neutral atoms, a crystal lattice has what kind of energy?
lower potential energy
The lattice energy is a measure of what?
strength of ionic bond
Compared with nonmetals, the number of valence electrons in metals is generally what?
Smaller
Define metallic bond.
A bond formed by the attraction between positively charged metal ions and the electrons around them
Ionic compounds are brittle because the strong attractive forces do what?
hold the layers in relatively fixed positions
What is one reason a metal has a shiny appearance?
mobile valence electrons within the structure
To appear shiny, a material must be able to do what?
absorbing and emitting light
Why are metals malleable?
because of the metallic bonding it allows the ions to slide past each other
A polar molecule contains what?
an area of positive charge, an area of negative charge
Compared with molecular bonds, the strength of intermolecular forces is what?
it is going to be weaker
The reason the boiling point of water (H2O) is higher than the boiling point of hydrogen sulfide (H2S) is partially explained by what?
hydrogen bonding
