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Name___________________________________ Per. ______ Electrons and Periodic Table (Ch. 4 & 5)

OTHS Academic Chemistry

Objectives: Express the arrangement of electrons in atoms through electron configurations

Understand the electromagnetic spectrum and the mathematical relationships between energy, frequency, and wavelength of light

Calculate the wavelength, frequency, and energy of light using Planck's constant and the speed of light

Explain the use of chemical and physical properties in the historical development of the Periodic Table

Use the Periodic Table to identify and explain the properties of the chemical families

Use the Periodic Table to identify and explain periodic trends

Vocabulary: electron configuration, frequency, amplitude, energy, wavelength, direct, inverse,

electromagnetic spectrum, energy level, sublevel, orbital, valence electron, octet, ion, cation, anion, electronegativity, ionization energy, atomic radius, ionic radius, period, group, shielding effect, transition metal, alkali metal, alkaline earth metal, metalloid, halogen, noble gas, lanthanide, actinide.

Topics to master: The electromagnetic spectrum

Wave calculations

Aufbau Principle vs. Pauli Exclusion Principle vs. Hund’s rule

Electron configurations

Orbital diagrams

Ion formation with dot diagrams

Periodic families and their properties

History of the periodic table- Mendeleev, Moseley, Seaborg

Periodic trends- Ionic & atomic radius, electronegativity, and ionization energy

CHECKLIST: How to be successful in OTHS Academic Chemistry

Pay attention and take notes in class Ask questions in class on material that is not clear Work every page in the practice packet for the unit Check answers to the practice packet online at http://othschem.weebly.com/ Come to tutorials with any chemistry teacher Do the online homework and check solutions once they become available Always do the practice test for every test & ask good questions on review day Keep up with the calendar for the class/be aware of approaching quizzes, tests, & other deadlines Use videos posted on website as a quick and convenient tutorial Read the chapter in the book

Provided: Periodic table c = f λ

c = 3.00 x 108 m/s

E = hf

h = 6.626 x 10 – 34 J . s

Wave Worksheet

Part 1

c = λ f c = speed of light = 3.00 x 108

m/s

wavelength (λ) should be expressed in meters (m)

frequency (f) should be expressed in reciprocal seconds (s-1 or Hz)

1. What is the frequency of radiation with a wavelength of 3.82 x 10-7 m? What part of the electromagnetic

spectrum does this fall in?

2. What wavelength of radiation has a frequency of 3.40 x 1018 Hz? What part of the electromagnetic spectrum

does this fall in?

3. What is the frequency of red light if the wavelength is 7.60 x 10-7 m?

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4. The green light associated with the aurora borealis is emitted by excited oxygen atoms. Its wavelength is

5.58 x 10-7 m? What is the frequency of this green light?

5. Gamma rays have frequencies around 1.0 x 1021 Hz. What wavelength does this correspond to?

Part 2

E = h f h = Planck’s constant = 6.626 x 10-34 J . s

6. How much energy does a photon of light with a frequency 4.2 x 108 Hz have? What part of the

electromagnetic spectrum does this fall in?

7. It takes 6.63 x 10-18 J of energy to eject an electron from a certain atom. What frequency of light is this?

What part of the electromagnetic spectrum does this fall in?

8. What is the energy of a photon of light with a wavelength of 6.10 x 10-7 m? Hint: you need to use the

equation from Part 1 also! What color is this light?

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Electron Configuration

1. Give the electron configuration for the following elements: ***The noble gas configuration can be used after oxygen

He ____________________ Si ____________________

Be ____________________ Ni ____________________

O ____________________ As ____________________

Na ____________________ Sn ____________________

Al ____________________ Bi ____________________

Ar ____________________ Ba ____________________

Sc ____________________ Cd ____________________

2. Identify the specific element (symbol) that has the following electron configuration:

ls2 2s2 2p1 ______ [Ne] 3s2 3p5 ______

[Ne] 3s2 3p3 ______ [Ar] 4s2 3d10 4p4 ______

[Ar] 4s1 ______ [Kr] 5s2 4d10 5p6 ______

[Ar] 4s2 3d10 ______ ls2 2s2 2p5 ______

[Kr] 5s2 ______ [Xe] 6s2 4f14 5d10 6p5 ______

[Ar] 4s2 3d10 4p2 ______ [Kr] 5s2 4d2 ______

[Xe] 6s1 ______ [Ar] 4s2 3d6 ______

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LEVELS, SUBLEVELS, ORBITALS, AND ELECTRONS

1. Which energy level

a. holds a maximum of eight electrons? ________

b. contains only an s sublevel? ________

c. is the first to have s, p and d sublevels present? ________

d. is the first to have a f sublevel? ________

2. Which sublevel(s) are present in

a. the first energy level? ________

b. the third energy level? ________

c. the fourth energy level? ________

3. How many orbitals are in

a. the first energy level? ________

b. the s sublevel in the second energy level? ________

c. the p sublevel in the fourth energy level? ________

d. the third energy level? ________

e. the d sublevel in the fifth energy level? ________

4. How many electrons (maximum number) may be placed in

a. the second energy level? ________

b. the s orbital in the fourth energy level? ________

c. the d sublevel in the third energy level?. ________

d. one f orbital? ________

e. a 3p orbital? ________

f. a 3p sublevel? ________

g. one p orbital? ________

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Ions

Ion Formation Worksheet

“The name’s Bond, Ionic Bond. I like my electrons taken, not shared.”

An ion is a charged particle formed by loss or gain of electrons. Atoms form ions in order to attain a stable octet (8 valence electrons) in the outer energy level.

When an atom LOSES electrons, this results in a positively charged ion (CATION).

When an atom GAINS electrons, this results in a negatively charged ion (ANION).

Element e- dot

structure

Lose or gain e-?

How many?

Ion formula

w/ charge

(1) Electron configuration of atom

(2) Electron configuration of ion

Mg

Mg

Lose 2

Mg2+

(1) Mg= 1s2 2s2 2p6 3s2 (2 valence e-)

(2) Mg2+= 1s2 2s2 2p6 (8 valence e-)

Al

S

Na

Cl

Ionic Compound Formation: Simple ionic compounds are formed when a metal loses electrons to a

nonmetal. Then the two newly formed + and – ions attract.

Complete electron dot diagrams for the following combinations, showing transfer of electrons with arrows.

(a) Mg and S

(b) Na and S

(c) Al and Cl

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SUMMARY OF PERIODIC AND GROUP TRENDS

TREND ATOMIC RADIUS / IONIC RADIUS

IONOZATION ENERGY / ELECTRONEGATIVITY

DOWN A GROUP ___________________________

Reason: Increasing Energy levels

___________________________

Reason: Increasing shielding effect ACROSS A PERIOD DECREASES

Reason: _______________________

_______________ _____________

INCREASES

Reason:__________________________

_______________ _______________

*Note: Noble gasses are NOTelectronegative! Fluorine (F) is the most electronegative element.

Write in the patterns that the trends follow on the periodic table below:

TRENDS IN IONIC RADIUS FOR THE SAME ELEMENT

A POSITIVE ion is a CATION. It is a METAL that has LOST electrons.

POSITIVE ions are SMALLER than the neutral atom.

Examples: Na+ is ________________ than Na

A NEGATIVE ion is an ANION. It is a NON-METAL that has GAINED electrons.

Negative ions are LARGER than the neutral atom.

Examples: F – is ________________ than F

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Worksheet: Periodic Trends Circle the correct answer

Atomic Radius

1. a. Atomic radius increases / decreases going down a group.

b. Atomic radius increases / decreases going left to right across a period.

2. a. Which element has the larger atomic radius?

i. Ca or Ba iii. Rb or Kii. Ca or Br iv. B or F

b. Which element has the smaller atomic radius?

i. Fe or Zn iii. Xe or Neii. Br or I iv. Na or Al

Ionic Radius

3. a. A positive ion (cation) like Na+ is always smaller / larger than the neutral metal atom (Na).

b. A negative ion (anion) like F – is always smaller / larger than the neutralnonmetal atom (F).

4. Which has the larger radius?

i. K or K+ iii. O or O 2-

ii. Ca or Ca2+ iv. Cl or Cl -

5. a. Ionic radius increases / decreases going down a group.

b. Ionic radius increases / decreases going left to right across a period.

6. Which has the smaller ionic radius?

i. Ca2+ or Ba2+ iii. Rb+ or Sr2+

ii. Cl - or Br - iv. N 3- or F -

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Ionization Energy 7. a. Ionization energy increases / decreases going down a group. b. Ionization energy increases / decreases going L to R across a period. 8. a. Which element has the greater ionization energy? i. Si or Cl iii. Ga or Br ii. Si or Pb iv. Li or Cs b. Which element has the smaller ionization energy? i. C or Sn iii. P or Bi ii. Ba or Au iv. Be or O

Electronegativity

9. a. Electronegativity increases / decreases going down a group. b. Electronegativity increases / decreases going L to R across a period. 10. a. Which element has the greater electronegativity? i. Cl or Al iii. N or As ii. K or Fr iv. Li or F

b. Which element has the smaller electronegativity?

i. Hg or Pb iii. Cr or W ii. Be or Ba iv. Sb or I

11. Group trends identified for the previous properties of the elements can be

explained by a particular principle, the ________________ ____________. (Use your notes to identify it!)

12. Periodic trends identified for the previous properties can be explained by another principle, increasing ________________ ___________. (Use your notes!)

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