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AP Chem Unit 2 TSNF

Terms in this set (36)

What is electronegativity?
a measure of the ability of an atom to attract shared electrons in a chemical bond
Which element has the highest electronegativity?
Fluorine (F)
What type of bonding occurs between metals and non-metals?
Ionic
What type of bonding typically occurs among non-metals?
Covalent
What type of bonding typically occurs within a metal?
Metallic
Which type of chemical bonding involves 2 atoms sharing some valence electrons?
Covalent
Which type of chemical bonding involves atoms transferring valence electrons?
Ionic
Which type of chemical bonding involves all the atoms sharing all their valence electrons?
Metallic
Describe the structure and properties of ionic solids
Crystal lattice, hard, rigid, does not conduct electricity
In which type of chemical bonding are valence electrons delocalized?
Metallic
What are some properties of metals?
- malleable
- ductile
- shiny (luster)
- high melting point
- good conductor of electricity
What properties indicate that an unknown substance may have ionic bonding?
High melting point, crystalline solid, conducts when melted or dissolved but not when solid
What properties indicate that an unknown substance may contain covalent bonding?
Low melting point, never conducts electricity
What is an ion?
A charged atom or molecule
How do you determine how many atoms are in an ionic compound's formula?
Balance the charges (make the total + and - charges equal and opposite)
How do you show ionic bonding in a Lewis structure?
Include the charges and/or brackets
How many valence electrons are shared in a single bond?
2
What is a bonding domain?
One single, double, or triple bond
What is a nonbonding domain?
One lone pair (2 unshared valence electrons)
In what order do you assign valence electrons to a Lewis structure?
1. Single bonds
2. Lone pairs on outside atoms
3. Lone pairs on center atom(s)
4. Change lone pairs to multiple bonds if needed
What does the "HONC Rule" tell you?
How many bonds an atom likely forms:
Hydrogen: 1 bond
Halogens: 1 bond, 3 lone pairs
Oxygen: 2 bonds, 2 lone pairs
Nitrogen: 3 bonds, 3 lone pairs
Carbon: 4 bonds
Which elements are exceptions to the octet rule? How many valence electrons can they have in molecules?
Hydrogen: 2
Beryllium: 4
Boron: 6
Elements in groups 3-7: usually 8, but can have more if needed
When would a molecule's center atom have an expanded octet?
If there are too many atoms (5+ atoms attached to center atom) or too many valence electrons
How can you tell a compound is covalent using its chemical formula?
It contains only nonmetals (and does not start with NH₄)
Which 5 transition and post-transition metals only get one charge each? What are their charges?
Ag⁺, Cd²⁺, Zn²⁺, Ga³⁺, Al³⁺
If an ion called "argentate" contained 4 oxygen atoms, how many oxygen atoms would "argentite" contain?
3 (-ite is 1 less oxygen than -ate)
What do we call the amount of energy needed to break an ionic bond?
Lattice energy/enthalpy
What two factors affect lattice energy?
Magnitude of charges and distance between charges
Which of these compounds has the greatest lattice energy: MgO, CaS, KCl, or NaF?
MgO, because the charges are stronger and the ions are smaller
What is a polar covalent bond?
A bond in which electrons are shared unequally between atoms with a medium electronegativity difference
What is a sigma bond?
The first bond between two atoms, which uses a hybridized orbital located directly between the two nuclei
What is a pi bond?
An additional (second or third) bond between two atoms, which uses p orbitals above and below the nuclei
What are the three possible hybridizations?
sp, sp², and sp³
How do you calculate the formal charge of an atom in a Lewis structure?
1. All unshared electrons belong to that atom
2. One electron from each shared pair belongs to that atom
3. Subtract (valence electrons according to PT) - (valence electrons assigned in structure)
If two Lewis structures both obey the octet rule, which is better?
The one with more formal charges of zero
What makes a molecule polar?
Asymmetrical distribution of charge in space (due to electronegativity differences and/or asymmetrical Lewis structure)
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