1
Consider the balanced equation: 3 H2(g) + O3(g) 3 H2O(g)
Given the following DHf values:
DHf for H2(g) = 0 kJ/mole
DHf for O3(g) = +143 kJ/mole
DHf for H2O(g)= -242 kJ/mole
What is the enthalpy of the reaction (ΔHrxn) above?
-869 kJ
Quantum theory is
A) a theory that unifies all strong and weak forces in nature.
B) a theory that focuses just on the particle nature of light.
C) a theory that focuses just on the wave nature of light.
D) a theory that unifies the wave-particle dual nature of electromagnetic radiation.
E) only applicable in outer space.
D) a theory that unifies the wave-particle dual nature of electromagnetic radiation.
A certain electromagnetic radiation has a wavelength of 125 nm (1nm = 1x10^-9m). What is the frequency of this electromagnetic radiation?
2.40x10^15 s-1
Which of the following wavelengths has the highest energy?
A) 445 nm
B) 189 nm
C) 116 nm
D) 245 nm
E) 389 nm
c) 116nm
If a 0.125 kg animal runs at 0.275 m/s, what is its de Broglie wavelength?
1.93x10^-32 m
What is the ΔE predicted when the electron in a H atom transitions from n=1 to n=4?
2.04x10^-18 J
According to the Heisenberg Uncertainty Principle, it is impossible to precisely know the location and ________ of an electron.
A) fluidity
B) affinity
C) speed
D) mass
E) charge
c) speed
Which of the following is NOT a valid set of quantum numbers?
A) n=2; l=0; ml = 0
B) n=3; l=2; ml = -1
C) n=2; l=1; ml = -1
D) n=2; l=1; ml = 0
E) n=4; l=4; ml = 2
E) n=4; l=4; ml = 2
Which of the following types of orbitals do NOT exist?
A) 1s
B) 4s
C) 1d
D) 2p
E) 3d
c) 1d
How many orbitals (ml values) are allowed in a subshell designated by n=3 and l=1?
3
What is the maximum number of electrons that can be contained in the n=4 principal quantum level?
32
The full electron configuration for Vanadium (V, atomic #23) is
1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^3
Based on periodic trends, which of the following elements is expected to have the largest first ionization energy?
A) Ca
B) Mg
C) Si
D) F
E) S
d) F
Which of the following is expected to be the most basic oxide?
A) Na2O
B) CO2
C) CaO
D) K2O
E) NO2
d) K2O
Draw the expected orbital diagram for Chlorine (Cl). How many unpaired electrons are there and would this be considered diamagnetic or paramagnetic?
1, paramagnetic
The element Manganese (Mn) is atomic number 25. The expected condensed electron configuration of the Manganese 2+ ion (Mn2+) is ___________.
[Ar] 3d5
Which of the following species in an isoelectronic series has the smallest radius?
A) Ne
B) F-
C) O2-
D) Na+
E) Mg2+
Mg2+
You did an experiment in the lab and found the following successive ionization energies corresponding to an element in the third row of the periodic table:
Based on this pattern of ionization energies, what is the identity of the element?
Al
You found a mystery element in period 2 we will call “X” with the Lewis dot symbol
X... (three e-)
Of the following choices, what element was it?
A) Be
B) B
C) C
D) N
E) O
B) B
Which of the following ionic compounds has the largest lattice energy, i.e., the hardest to break apart?
A) MgS
B) RbBr
C) KBr
D) CaS
E) SrS
A) MgS
Which of the following bonds would have the highest bond energy?
A) C-C
B) C=C
C) C≡C
D) All are the same bond energy
C) C≡C
Based on electronegativity trends, which of the following bonds would you expect to be the most ionic in character?
A) Cl-S
B) Cl-P
C) Cl-Si
D) Cl-Al
E) Cl-Cl
d) Cl-Al
Given the bond energies (BE) below, what is the enthalpy change (ΔHrxn) for the following reaction: (draw on board)
-1282 kJ
What is the enthalpy change for the following target reaction (ΔHrxn) using Hess’s Law.
Target: C3H8(g) + 5 O2(g) 3 CO2(g) + 4 H2O(g)
Given:
-2044 kJ
Which of the following is an electron configuration of an excited state of an atom?
A) 1s^2 2s^2 2p^6 3s^1
B) 1s^2 2s^2 2p^6 3s^2 4s^1
C) 1s^2 2s^2 2p^6 3s^2 3p^6 4s^1
D) 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^3
B) 1s^2 2s^2 2p^6 3s^2 4s^1