# Instructions for using this template. Remember this is Jeopardy, so where I have written “Answer” this is the prompt the students will see, and where.

## Presentation on theme: "Instructions for using this template. Remember this is Jeopardy, so where I have written “Answer” this is the prompt the students will see, and where."— Presentation transcript:

Instructions for using this template. Remember this is Jeopardy, so where I have written “Answer” this is the prompt the students will see, and where I have “Question” should be the student’s response. To enter your questions and answers, click once on the text on the slide, then highlight and just type over what’s there to replace it. If you hit Delete or Backspace, it sometimes makes the text box disappear. When clicking on the slide to move to the next appropriate slide, be sure you see the hand, not the arrow. (If you put your cursor over a text box, it will be an arrow and WILL NOT take you to the right location.)

Choose a category. You will be given the answer. You must give the correct question. Click to begin.

Orbitals & electrons Misc.Calculations 10 Point 20 Points 30 Points 40 Points 50 Points 10 Point 20 Points 30 Points 40 Points 50 Points 30 Points 40 Points 50 Points Electron Configuration Scientists

Created the “planetary” model of the atom

Bohr

Told us that you cannot know, with any degree of certainty, both the location of an electron as well as its velocity at any given instant.

Heisenberg

Developed an equation that allows us to predict the energy either admitted or absorbed by an electron if we know the final and initial energy levels for the electron’s jump.

Rydberg

Assumed that energy can either be absorbed or released by atoms in discrete “chunks” which he called quantums

Planck

Developed a wave equation which allows us to predict the likelihood (probability) of finding an electron in a general region of space around the nucleus

Schrodinger

How many orbitals are required in each subshell- s? p? d? f?

s-1, p-3, d-5, f-7

What family has an electron configuration that ends with s 2 ?

Alkaline earth metals

Describe the shape of the 5 th d orbital (the one that no one likes to talk about)

2 lobes and a donut

How many electrons can each energy level hold in total? n=1? n=2? n=3? n=4?

n=1 – 2 e- n=2 – 8e- n=3 – 18 e- n=4 – 32 e-

What is the vocab word used to describe orbitals of equal energy?

Degenerate

Give the standard configuration for sulfur.

1s 2 2s 2 2p 6 3s 2 3p 4

Give the Noble gas configuration for antimony

[Kr]5s 2 4d 10 5p 3

Draw an orbital diagram for strontium

See board

Give the Noble gas configuration for tungsten

[Xe]6s 1 4f 14 5d 5

Write the standard configuration for uranium

1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10 6p 6 7s 2 5f 4

Color in the visible spectrum with the shortest wavelength

violet

Type of electromagnetic radiation with waves the length of a football field

Relationship between frequency and wavelength

inverse or indirect

The transition below with the lowest energy photon EMISSION n= 1  n = 6 n = 6  n = 3 n = 1  n = 4 n = 6  n = 2

n = 6  n = 3

The name for the phenomena that says every metal has a minimum frequency of light below which no electrons are emitted, and that the intensity of this light is not a crucial factor

Photoelectric effect

Convert 588 nm to meters.

5.88x10 -7 m

Your favorite radio station broadcasts at a frequency of 1.15x10 6 Hz or s -1. What is this wavelength in centimeters?

26,087 cm

Calculate the frequency of a photon with an energy of 1.66x10 -17 J.

2.5x10 16 s -1 or Hz

Calculate the change in energy when an electron jumps from n=4 to n=1 in a hydrogen atom.

-2.04x10 -18 J

Calculate the wavelength of a photon absorbed in a hydrogen atom when an electron jumps from n=3 to n=6.

1.09x10 -6 m