Wavelength, Frequency and Energy
Electron Shells, Subshells and Orbitals
Orbital Diagrams and Electron Configurations
Periodic Trends
The Mole
100
The wavelength of light in nm, when a laser emits light of a frequency of 4.35 x 1014 Hz.
What is 6.90 x102 nm?
100
The electrons in the outermost electron shell of the atom are called this?
What are the valance shell electrons?
100
The number of unpaired electrons in osmium.
What is 5?
100
Rank the following in increasing first ionization energy.
C, Si, Ga
What is:
Ga < Si < C
100
200. g of NaCl. How many moles of NaCl is this?
(Molar mass NaCl = 58.44 g/mol)
What is 3.42 moles?
200
Electromagnetic radiation travels through vacuum at a speed of __________ m/s.
3.00 x 108 m/s
200
The number of subshells in n = 7?
What is 7 subshells?
200
The element that has the electron configuration 1s2 2s2 2p2.
What is Carbon?
200
Arrange the following ions in order of increasing radius: F- , Na+ , O2-, Mg2+, N3-
What is:
Mg²⁺ < Na⁺ < F⁻ < O²⁻ < N³⁻
200
How many molecules are in 88 g of CO₂?
(Molar mass CO₂ = 44.01 g/mol)
What is 1.2 × 1024 molecules?
300
Calculate the energy of light with a frequency of 6.00 × 10¹⁴ Hz.
What is 3.98 × 10⁻¹⁹ J?
300
The number of orbitals in a 5f subshell
What is 7 orbitals?
300
The noble gas configuration of tin and predict the two most common ions that tin will form.
Sn:
[Kr]5s24d105p2
+2 and +4 ions
300
Explain why atomic size increases as you go down a group.
What is:
Atomic size increases as you go down a group because additional energy levels (electron shells) are added.
300
How many molecules are in 11.2 L of CH4 at STP?
What is 3.01×1023 molecules?
400
Calculate the energy of a photon with a wavelength of 4.00 × 10-7 m.
What is 4.97 × 10-19 J?
400
The total number of electrons that n = 4 can hold
What is 32 electrons?
400
Refer to the first three ionization energies of four period 3 elements. The elements are randomly assorted.
Identify Element 3 and its complete electron configuration.
What is Mg and 1s22s22p63s2
400
Explain why ionization energy increases as you move across a period.
What is:
Ionization energy increases across a period because the number of protons increases while electrons are added to the same energy level, causing a stronger attraction between the nucleus and the valence electrons and making them harder to remove.
400
What mass of He gas is in 11.2 L at STP?
(Molar mass He = 4.00 g/mol)
What is 2.00 g?
500
The energy of a particular color of green light is 3.82 x 10-22 kJ. What is its wavelength in nanometers?
What is 520. nm?
500
The number of orbitals and electrons in n = 5
What is 25 orbitals?
500
Use the whiteboard.
Draw the highest energy subshell (with electrons) for iron.
500
Refer to the first three ionization energies of four period 3 elements. The elements are randomly assorted.
What is the symbol and most common ion formed by Element 2?
Na and +1
Also accept Na+1
500
A 5.0 L sample of helium gas is collected at 2.0 atm and 300 K. What is the mass of the helium gas?
What is 1.62 g He?