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# Unit 2 Extra Practice PowerPoint PPT Presentation

Unit 2 Extra Practice. October 15 (ODD) October 16 (EVEN). Do Now (5 min). How much energy is given off by an electron emitting a wave with a frequency of 7 x 10 14 Hz? As the wavelength of light increases, The frequency increases The speed of light increases The energy decreases

Unit 2 Extra Practice

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## Unit 2 Extra Practice

October 15 (ODD)

October 16 (EVEN)

### Do Now (5 min)

• How much energy is given off by an electron emitting a wave with a frequency of 7 x 1014 Hz?

• As the wavelength of light increases,

• The frequency increases

• The speed of light increases

• The energy decreases

• The intensity increases

Justify your answer with a diagram. Use p. 139 as needed.

### Announcements

• OWN Your Education

• Office hours Wednesday and Friday

• All makeup work due Monday 10/22

• Unit 2 exam and quiz schedule:

## Review Questions

If you work efficiently, we may have time to play a jeopardy game at the end of class 

## Bohr Model vs. Quantum Model Questions (10 min)

Answer the questions from the sheet on a separate sheet of paper that you will turn in at the end of class.

• (5 min)

• How many electrons are needed to fill the first, second, and third principal energy levels in the Bohr Model of the atom?

• Draw the Bohr Models for Aluminum and Neon.

• What is an “orbital” (in the Quantum Mechanical Model)? How is it different than an “orbit” (in the Bohr Model)?

• How does the Bohr Model of the atom differ from the Quantum Mechanical Model? List at least three ways.

• (5 min)

• How many electrons can fit into the s, p, and d sublevels? How is this information shown on the periodic table?

• How many orbitals do the s, p, d, and f sublevels have? What is the relationship between the number of orbitals a sublevel has and the number of electrons that sublevel can hold?

• How is the amount of an energy an electron has related to the orbit(al) that electron is in (in both the Bohr Model and Quantum Mechanical Model of the atom)

## Electron Configuration Questions (10 min)

Answer the questions from the sheet on a separate sheet of paper that you will turn in at the end of class.

• (5 min)

• Make a rough sketch of the periodic table and label the different sections: s, p, d, and f.

• What do the 1, s, and 2 mean, respectively, in this electron configuration: 1s2?

• Write electron configurations for the following elements: Lithium, Carbon, Neon, Silicon, Iron.

• (5 min)

• Write the Noble Gas Configuration (shortcut) configurations for Silicon and Iron.

• Write electron configurations for elements with the following numbers of electrons: 4, 7, 16.

• Where on the periodic table would you expect to find an element whose ground-state electron configuration ended in 4p5? 3s1?

## Orbital Diagram Questions (10 min)

Answer the questions from the sheet on a separate sheet of paper that you will turn in at the end of class.

• How many boxes do the s, p, and d sublevels get? How do these numbers compare to the number of orbitals in those sublevels?

• Identify the problem in each of the following orbital diagrams. Which rule(s) is(are) being violated?

• Write the symbol for the elements with the following orbital diagrams:

How many unpaired electrons (single electrons in an orbital) do each of the following elements have: Na, Ca, O?

## Groups, Families and Valence Electron Questions (10 min)

Answer the questions from the sheet on a separate sheet of paper that you will turn in at the end of class.

• How is the Periodic Table organized?

• Describe in 5 words or less where to find each of the following on the periodic table: Metals, Nonmetals, Metalloids (semi-metals).

• List three common physical properties of metals. Do the same for nonmetals.

• Match the following families (groups) to their columns on the periodic table:

• Halogens

• Noble Gases

• Alkali Metals

• Alkaline Earth Metals

• Transition Metals (list the range of columns)

• Are the elements in a group (column) or period (row) on the periodic table more similar to each other? Explain.

• How does reactivity change as you go down the periodic table? Which element is more reactive than potassium, but less reactive than Cesium?

• What family would elements with the following electron configuration belong to:

• 1s22s2

• 1s2 2s2 2p5

• 1s2 2s2 2p6

• [Ne] 3s1

• [Ne] 3s2 3p6

• [Ar] 4s2 3d6

• What is a valence electron? Where can you look on the periodic table to figure out how many valence electrons an element has?

• How many valence electrons do the following elements have: Sodium, Calcium, Neon, Fluorine, Chlorine, Oxygen, Phosphorous?

## Periodic Trends Questions (10 min)

Answer the questions from the sheet on a separate sheet of paper that you will turn in at the end of class.

### Periodic Trends Questions

Define electronegativity, atomic radius, and ionization energy.

How does electronegativity vary from left to right on the periodic table?

How does atomic radius vary across a period and down a group in the table?

Which two atomic properties have similar trends? Offer a possible explanation for this similarity.

Why do noble gases have the highest ionization energy?

Which is more reactive? Lithium or Potassium? Oxygen or Fluorine?

## Electromagnetic Spectrum Questions (10 min)

Answer the questions from the sheet on a separate sheet of paper that you will turn in at the end of class.

### Electromagnetic Spectrum

Write the equation relating the speed of light with frequency and wavelength. Write the equation relating energy and frequency. Label the variables in each.

The speed of light always equals ____________.

Answer questions #11-14 on p. 157.

Which has more energy, a radio wave or a gamma ray?

If a radio wave has a frequency of 106 Hz, what is its wavelength? How much energy does it carry?

If purple light has a wavelength of 4.00 x 10-7 m, how much energy does it have?

Unit 2 Review

### POWERPOINT JEOPARDY

Atom Models

Electron Configuration

Orbital Diagram

Periodic Table/Trends

Electromagnetic Spectrum

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Name the 4 orbitals and describe the shapes – 10 Points

Sodium (Na) has how many electrons in the third energy level? – 20 Points

Copper has how many electrons in the 3d sublevel? – 30 Points

Draw the Bohr model for Argon (Ar)– 40 Points

Draw the quantum model for Neon– 50 Points

What is the electron configuration for Neon (Ne) – 10 Points

Write the electron configuration for an element that would have 14 protons – 20 Points

Silicon has an electron configuration of 1s22s22p63s23p2. How many electrons does silicon have in its highest sublevel? – 30 Points

Write the electron configuration for Bromine (Br) – 40 Points

Which element would have the following shortcut electron configuration: [Ar]4s23d104p4– 50 Points

Which rule is being violated in the orbital diagram below? – 10 Points

Which element is represented by the following orbital diagram – 20 Points

Which rule is being violated in the orbital diagram below? – 30 Points

Which rule is being violated in the orbital diagram below?– 40 Points

Draw the orbital diagram for Silicon – 50 Points

What are the rows and columns called in the periodic table – 10 Points

Which has the greater Ionization Energy? Electronegativity? Atomic radius? Fluorine or Oxygen?– 20 Points

If I am an element that is shiny, hard, and a good conductor of heat and electricity, what kind of element am I? – 30 Points

If I react vigorously with water, what family am I in and where can you find me on the periodic table and how many valence electrons do I have? – 40 Points

What family does the following element belong to and how many valence electrons does it have: 1s22s22p63s23s5– 50 Points

What is the wavelength for a wave with a frequency of 2 x 103 Hz– 10 Points

What is the frequency for a wave with a wavelength of 100 m – 20 Points

What is the energy if the frequency is 4 x 1010 Hz? – 30 Points

What is the frequency if the energy is 2 x 10-19?– 40 Points

What is my energy if my wavelength is 300 m– 50 Points