Subatomic Particles
How do isotopes differ from each other? Ions?
Isotopes of the same element have different number of neutrons. Ions have different number of electrons.
What is the relationship between wavelength, frequency, and energy?
Wavelength is inversely related to frequency and energy. Frequency and energy are directly related.
Briefly describe the quantum numbers:
n l ml ms
*Hint: what do the numbers tell you about an electron's location?
n- shell
l - shape
ml- orbital
ms- spin direction
How do electrons fill up orbitals?
Electrons fill orbitals one at a time and in the same direction. If more electrons need to be placed, electrons fill in those orbitals in the opposite direction.
Briefly explain the atomic size trend.
**Hint: What happens when you go down a column and move to the left on the periodic table?
Moving down a column: Gaining more rings
Left of the periodic table: Less outer electrons, less nuclear charge
Write the nuclide symbol for an atom with
31 protons, 31 electrons, 39 neutrons
3170Ga
With a wavelength of 532 nm, a photon has a frequency of _s-.
5.64 x 1014
Below is an incomplete set of quantum numbers
n= 4 l =2 ml=? ms= +1/2
The possible values for ml are _.
-2, -1, 0, 1, 2
What element belongs to each electron configuration?
A) 1s2 2s2 2p2
B) 1s2 2s2 2p6 3s2 3p4
C) 1s2 2s2 2p6 3s2 3p6 4s2 3d7
D) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5
A) Carbon
B) Sulfur
C) Cobalt
D) Bromine
This is the proper ranking of F, Mg, Ca based on increasing electronegativity is _.
Ca, Mg, F
Break down the following atoms into their sub-particles:
Carbon-13
Neon-21
1735Cl-1
3479Se-2
37Li+
C - 6 p 6 e 7 n
Ne - 10 p 10 e 11 n
Cl - 17 p 18 e 18 n
Se - 34 p 36 e 45 n
Li - 3 p 2 e 4 n
A particle emits 2.67 x 10-18 J. The wavelength of this photon is _nm.
74.4
Which is a correct set of quantum numbers?
A) n= 3 l= 2 ml= -1 ms= +1/2
B) n= 1 l= 1 ml= +1 ms= +1/2
C) n= 2 l= 1 ml= 0 ms= +1
D) n= 4 l= 2 ml= 0 ms= -1/2
A and D
Write the element and its ion's configurations
A) Scandium and Sc+
B) Phosphorus and P3-
C) Nickel and Ni 2+
D) Rubidium and Rb+
Sc [Ar] 4s2 3d1 and [Ar] 4s13d1
P [Ne] 3s2 3p3 and [Ne] 3s2 3p6
Ni [Ar] 4s2 3d8 and [Ar] 3d8
Rb [Kr] 5s1 and [Kr]
Rank the following based on increasing:
Size: Se Al Si
Affinity: K Br C
Ionization Energy: Mg Ti P
Size: Se< Si< Al
Affinity: K< C< Br
IE: Mg< Ti<P
What charges do elements in the following groups take?
Alkaline Earth Metal
Alkali Metal
Nobel Gas
Transition Metals
Halogen
AEM +2
AM +1
NG 0
TM It depends!
Halogen -1
An electron transitions from n = 2 to n = 3. Calculate the energy, frequency, and wavelength associated with this transition.
Energy = 3.03 x 10-19 J
Wavelength = 6.56 x 10-7 or 656 nm
Frequency = 4.57 x 1014 s-
How many electrons can the following the following hold?
A) n= 2 l= 1
B) n= 3 l=0
C) n= 3 l= 2
D) n= 4 l= 1 ml= +1
A) 6
B) 2
C) 10
D) 2
Which electron has the most unpaired electrons?
A) Mg
B) Cl
C) Zn
D) N
Nitrogen (3)
The largest alkali earth metal _ has a (smaller/larger) electronegativity than the largest halogen _.
Radium, smaller, Iodine
Which isotope has the largest number of neutrons?
a. Oxygen-18
b. Carbon-12
c. Fluorine-18
d. Nitrogen-14
Oxygen-18
Photon A transitions from n=1 to 2. Photon B transitions from n=4 to 3. Photon C transitions from 5 to 2. Draw this on an energy diagram. Arrange in order of increasing wavelength.
*Hint: you don't need to calculate wavelength or energy!
A<C<B
Boron's last electron is in the 2p orbital. What are the quantum numbers for this electron?
n = 2
l = 1
ml = -1
ms = +1/2 or -1/2
Given the quantum numbers of the last electron of an element
n = 2 l = 1 ml= 0 ms= -1/2
The element the electron belongs to is_
Fluorine
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