Chemistry ch. 2 & 3
How many orbitals are contained in the third principal level (n = 3) of a given atom?
9
Predict the charge that an ion formed from sulfur would have.
2-
What is the energy of light associated with a transition from n=3 to n=8 in a hydrogen atom? Does this represent absorption or emission of a photon?
2.08 × 10-19 J, absorption
It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy for an atom of hydrogen, making the assumption that ionization is the transition from n=1 to n=infinity
+2.18 × 10-18 J
Give the possible values for ml for a d orbital
-2, -1, 0, 1, 2
Determine the energy change associated with the transition from in the hydrogen atom.
-3.03 × 10-19 J
Calculate the energy of the red light emitted by a neon atom with a wavelength of 703.2 nm
2.83 × 10-19 J
Calculate the wavelength (in nm) of the blue light emitted by a mercury lamp with a frequency of 6.88 × 1014 Hz
436 nm
Give the number of core electrons for Cd.
46
Calculate the wavelength of a football (425 g) thrown by an NFL quarterback traveling at 50 mph.
6.97 × 10-26 nm
Determine the shortest frequency of light required to remove an electron from a sample of Ti metal, if the binding energy of titanium is 3.14 × 103 kJ/mol.
7.87 × 1015 Hz
Identify the number of valence electrons in Cl-.
8
Choose the statement that is TRUE.
Core electrons effectively shield outer electrons from nuclear charge.
Choose the valence orbital diagram that represents the ground state of Sr2⁺.
D
No two electrons can have the same four quantum numbers is known as the
Pauli exclusion principle.
Which of the following types of waves are considered electromagnetic radiation:
Radio Waves and Microwaves
Which reaction below represents the second electron affinity of S?
S⁻(g) + e⁻ → S2⁻(g)
Which of the following statements is FALSE?
The alkali metals are fairly unreactive.
Which of the following statements is TRUE?
The emission spectrum of a particular element is always the same and can be used to identify the element. B) Part of the Bohr model proposed that electrons in the hydrogen atom are located in "stationary states" or particular orbits around the nucleus. C) The uncertainty principle states that we can never know both the exact location and speed of an electron. D) An orbital is the volume in which we are most likely to find an electron. E) All of the above are true.
Which of the following statements is FALSE?
The halogens tend to form 1+ ions.
Which of the following statements is TRUE?
The magnetic quantum number (ml ) describes the orientation of the orbital
Which of the following occur as the energy of a photon increases?
The wavelength gets shorter.
Which of the following elements is an actinide?
U
Which element is diamagnetic?
Zn
Choose the ground state electron configuration for Zn2⁺.
[Ar]3d10
Give the ground state electron configuration for Se2⁻.
[Ar]4s23d104p6
Give the ground state electron configuration for Pb.
[Xe]6s24f145d106p2
For a given atom, identify the species that has the smallest radius.
cation
The element that corresponds to the electron configuration 1s22s22p63s23p64s13d5 is
chromium
When waves of equal amplitude from two sources are out of phase when they interact, it is called
destructive interference
When a wave encounters an obstacle or a slit that is comparable in size to its wavelength, it bends around it. This characteristic is called
diffraction
If two electrons in the same atom have the same value of "l", they are
in the same sublevel, but not necessarily in the same level.
According to the Heisenberg Uncertainty Principle
you cannot accurately know both the position and momentum of an electron at the same time.
Calculate the wavelength of an electron (m = 9.11 × 10-28 g) moving at 3.66 × 106 m/s
1.99 × 10-10 m
Calculate the wavelength of light emitted from a mol of photons as they transition from n=6 to n=3 in the hydrogen atom.
1093 nm
Give the complete electronic configuration for Mn.
1s22s22p63s23p64s23d5
How many nodes are found in a 3s orbital?
2
How many sublevels are contained in the second shell (n = 2) of a given atom?
2
How many orbitals are associated with an atom when n=5?
25
How many 8p orbitals exist?
3
What value of l is represented by an f orbital?
3
Calculate the frequency of light associated with the transition from n=2 to n=3 in the hydrogen atom
4.57 × 1014 s-1
How many photons are contained in a flash of green light (525 nm) that contains 189 kJ of energy?
4.99 × 1023 photons
Choose the valence orbital diagram that represents the ground state of Zn
A
Which of the following statements is TRUE?
An orbital that penetrates into the region occupied by core electrons is less shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy
Place the following in order of increasing IE1. N F As
As < N < F
Which of the following statements is TRUE?
Atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they take on a spherical shape.
Which element has the highest first ionization energy?
Cl
Place the following elements in order of increasing atomic radius. P Ba Cl
Cl < P < Ba
A scientist shines light with energy greater than the binding energy of platinum on a thin film of it. The same scientist then repeats the experiment with a higher intensity light. According to the photoelectric effect, what should be observed?
Electrons are ejected in both experiments at the exact same time.
Why does an electron found in a 2s orbital have a lower energy than an electron found in a 2p orbital in multielectron systems?
Electrons in the 2s orbital can penetrate the 1s orbital and be closer to the nucleus.
When filling degenerate orbitals, electrons fill them singly first, with parallel spins is known as
Hund's rule
Which ion has the largest radius?
K+
Which species has the highest ionization energy?
Mg2+
Place the following in order of increasing metallic character. Rb Cs K Na
Na < K < Rb < Cs
Place the following in order of increasing radius. Br⁻ Na⁺ Rb⁺
Na⁺ < Rb⁺ < Br⁻
Which reaction below represents the first ionization of O?
O(g) → O⁺(g) + e⁻
Which of the following quantum numbers describes the orientation of an orbital?
magnetic quantum number
Semiconductors are
metalloids.
What are the possible orbitals for n = 3?
s, p, d