Lewis Structures and Bonding
When electrons are not shared evenly between two atoms in a bond due to the difference in electronegativity, that bond is said to be ________.
Polar
This is the term for the tendency of an atom to attract electrons in a chemical bond
Electronegativity or Electron affinity
What is the electron domain geometry of a molecule that has 6 electron domains
octahedral
Pressure is also known as a _______ applied to a(n) _______.
force, area
How many orbitals are in the 4th sub-shell?
9 (1-s, 5-d, 3-p)
Draw the Lewis structure for water (H₂O), including lone pairs.
O in the center with 2 single bonds to H atoms
2 lone pairs on the O
Structure resembles a bent shape
What is the equation for the electron affinity of the chlorine (Cl) atom
Cl + e- → Cl-
Bonds that arise from orbital overlap across the internuclear axis are ________, and those that overlap above and below this axis are ___________
sigma-bonds, pi-bonds
You leave a basketball in the garage overnight during winter. The next morning, it's noticeably deflated. Later that day, after bringing it inside, it expands and feels firm again—even though you didn’t add any more air. What gas law is responsible for this observation?
Charles' Law
Why to atoms ionize (gain or loose electrons)?
To become iso-electronic with the noble gases
Draw the correct Lewis structure for sulfur hexafluoride (SF₆), including all lone pairs. Is this a polar molecule?
Sulfur (S) in the center
Six single bonds to six fluorine (F) atoms arranged octahedrally
Each fluorine has three lone pairs
Sulfur expands its octet to accommodate 12 electrons
It is non-polar
Put the following elements in order of increasing atomic radius: Oxygen (O), Sulfur (S), and Selenium (Se).
O < S < Se
This hybridization is typically associated with molecules exhibiting a trigonal planar molecular geometry.
sp2
An aerosol spray can with a volume of 125 mL contains 1.30 g of propane gas (C3H8, MM = 44 g/mol) as a propellant.
If the can is at 25 °C, what is the pressure in the can?
PV = nRT, R = 0.08206 L-atm/mol-K
5.77 atm
What element does the following electron configuration represent?
[Kr] 5s² 4d¹⁰ 5p⁵ → ?
Iodine (I)
Using the average bond enthalpies below, calculate the approximate enthalpy change (ΔH) for the following reaction:
CH₄ + Cl₂ → CH₃Cl + HCl
C–H = 412 kJ/mol, Cl–Cl = 243 kJ/mol, C–Cl = 328 kJ/mol, H–Cl = 431 kJ/mol
ΔH = –104 kJ/mol
Given the following elements: Aluminum (Al), Phosphorus (P), and Sulfur (S), rank them in order of decreasing first ionization energy.
P > S > Al
What is the electron domain and molecular geometry of the following geometry ClF3
EDG: Trigonal Bipyramidal
MG: T-shaped
A balloon inflated with He is rising into the atmosphere, based on Boyle's Law would you expect the balloon to increase or decrease in size?
What is the electron configuration of the Magnesium ion (Mg2+). What noble gas is it isoelectronic with?
1s22s22p6, Neon
Draw the resonance structures for the nitrate ion (NO₃⁻). Be sure to include charges on atoms as needed
Three structures with one double bond rotating among the three oxygen atoms
Each O not double-bonded has a negative charge
Total of 24 valence electrons used
Write the equations for the first 3 ionization energies of the Aluminum (Al) atom.
1. Al → Al+ + e-
2. Al+ → Al2+ + e-
3. Al2+ → Al3+ + e-
What is the electron domain and molecular geometry of the following molecule, XeF2
EDG: Trigonal Bipyramidal
MG: Linear
A gas occupies 8.50 L at a pressure of 874 torr and a temperature of 30 °C. Using the Ideal Gas Law, calculate the number of moles of gas in the container.
(PV=nRT, R = 0.0821 L·atm/mol·K; 1 atm = 760 torr)
0.393 moles
What is the condensed electron configuration of Indium (In)?
[Kr]5s24d105p1