Student Worksheet for Atomic Structure and Periodicity · 2017-06-18 · Student Worksheet for...

Advanced Chemistry Atomic Structure and Periodicity

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Student Worksheet for Atomic Structure and Periodicity

Attempt to work the following practice problems after working through the sample problems in

the videos. Answers are given on the last page(s).

Relevant Equations

E= h * f = ℎ𝑐

𝜆

c= 2.998*108 m/s

h= 6.626*10-34 Js

Where E= energy, s= second, J= Joules, h= Planck’s constant, f= frequency (per second), c= speed of

light, and λ= wavelength

Rules of Quantum Sets:

n= energy level

ℓ = range of 0-n

mℓ = range from – ℓ to + ℓ including 0

ms = +/ - ½

When filling quantum sets and counting across the periodic table, note that the value of mℓ goes in

increasing order.

When determining the ms, all + ½ values are completed prior to – ½ values.

When ℓ Equals Electron Orbital Is

0 S

1 P

2 D

3 F



1. Find Selenium (Se) on your periodic table and complete the following diagram.

What does each box represent?

A. _____________________________________________________________________________

B. _____________________________________________________________________________

C. _____________________________________________________________________________

2. Explain how your Box answer to 1a) is an accurate reflection of atomic isotopes.

3. Provide the long hand electron configurations for each of the following atoms:

Cl: _________________________________________________________________________________

Li: _________________________________________________________________________________

Cs: _________________________________________________________________________________

4. Provide the arrow electron configurations for each of the following atoms:

Na: _________________________________________________________________________________

N: __________________________________________________________________________________

Ar: __________________________________________________________________________________

Se 78.96

34

A.

B.

C.



5. Explain why (0, -1, 0, - ½ ) is not an allowable quantum configuration.

6. Identify each of the following atoms by quantum set:

(1,0,0, ½ ) ________________________________________________

(3, 1, -1, - ½) ______________________________________________

(4, 2, 0, ½ )_______________________________________________

7. Give the quantum set for each of the following atoms:

C: ____________________________________

Sr: ____________________________________

As: ___________________________________

8. Complete the following table:

Atom # of Electrons It Has # of Bonds It Makes

Ca

S

N

Ar

F

9. For each of the following atoms, draw the Lewis Dot Structure:

C P I



Draw the Lewis Dot Structures for each of the compounds in Questions 10-12:

10. C2H5OH

NH2OH

HBr

11. CH3CHO

H2CCHCOOH



12. C2H2

H3CCCCHCH2

13. It is known that there is a direct correlation between electronegativity and ionization energy. Explain

this relationship.

14. Calculate the amount of energy released at 200 nm.

15. At what frequency and wavelength will light emit 1.5*10--27 J of energy?



16. Fun Food for Thought that is very exciting. Given the following equations used in Physical Sciences

(including Chemistry and Physics), attempt to derive a relationship between Einstein’s E= mc2 and

Planck’s constant regarding light waves.

E = ℎ𝑐

𝜆

𝜆 = ℎ

𝑚𝑣



1. Find Selenium (Se) on your periodic table and complete the following diagram.

What does each box represent?

A. _The atomic weight is the number of protons + the sum of neutron abundances (isotopes exist when

a different number of neutrons exist in the same atom).

B. _The symbol is the 1-2 letter abbreviation of each atom on the periodic table

C. The number of protons in the atom.

2. Explain how your Box answer to 1a) is an accurate reflection of atomic isotopes.

When determining the mass of the atom, isotopes are averaged. To calculate the average, the

abundance for each atom is considered because the most accurate reflection is only based on how

common it is. For example, consider Carbon. 12C (Carbon 12) is present in 98.93%. 13C is present in

1.07%. 14C is present in trace amounts that can not be measured. Thus, C’s weight is calculated as

(12*0.9893) + (13*0.0107) = 12.011 rounded. The 13C has to be factored to account for its known

presence.

3. Provide the long hand electron configurations for each of the following atoms:

Cl: 1s22s22p63s23p5

Li: 1s22s1

Cs: 1s22s22p63s23p63d104s24p64d105s25p66s1

4. Provide the arrow electron configurations for each of the following atoms:

Se 78.96

34

A. Atomic Weight

B. Atomic Symbol

C. Atomic Number



5. Explain why (0, -1, 0, - ½ ) is not an allowable quantum configuration.

The ℓ value must be 0 or positive, up to the value of n. This ℓ is a negative number, which is not a

possibility to annotate an orbital.

6. Identify each of the following atoms by quantum set:

(1,0,0, ½ ) ____Hydrogen__________________________________

(3, 1, -1, - ½) _____Sulfur___________________________________

(4, 2, 0, ½ )______Niobium_________________________________

7. Give a quantum set for each of the following atoms:

C: ___(2, 1, 0, ½ )_________________________

Sr: ___(5, 0, 0, - ½ )_______________________

As: ___(4, 1, 1, ½ )_________________________

8. Complete the following table:

Atom # of Valence Electrons It Has # of Bonds It Makes

Ca 2 2

S 6 2

N 5 3

Ar 8 0

F 7 1



9. For each of the following atoms, draw the Lewis Dot Structure:

C P I

C P I

Draw the Lewis Dot Structures for each of the compounds in Questions 10-12:

10. C2H5OH

NH2OH

HBr



11. CH3CHO

H2CCHCOOH

12. C2H2



H3CCCCHCH2

13. It is known that there is a direct correlation between electronegativity and ionization energy. Explain

this relationship.

Electronegativity is the likelihood of an atom to pull an electron from another atom. Meaning that the

more electronegative that an atom is, the faster it will remove an electron from another atom. It’s

similar to Tug of War, and electronegativity is how strong the person/atom is. The rope is the electron.

Ionization energy is the amount of energy that is required to remove the electron. Going back to the Tug

of War example, the atom that needs less energy to pull the rope/electron away is more likely to lose it.

As you proceed from left to right across the periodic table, it becomes harder and harder for an electron

to be lost from those atoms. Hence, the ionization is higher and they are less likely to lose an electron.

We will revisit this concept in the Chemical Bonding unit.

14. Calculate the amount of energy released at 200 nm wavelength.

E= ℎ𝑐

𝜆

= ( 6.626∗10−34∗2.998∗108)

200

= 9.92*10-28 J

15. At what frequency and wavelength will light emit 1.5*10--27 J of energy?

E= h*f You are solving for f.

f= 𝐸

ℎ

= 1.5∗ 10^−27

6.626∗10^−34

= 2.26 * 106 waves/s



16. Fun Food for Thought that is very exciting. Given the following equations used in Physical Sciences

(including Chemistry and Physics), attempt to derive a relationship between Einstein’s E= mc2 and

Planck’s constant regarding light waves.

E = ℎ𝑐

𝜆

𝜆 = ℎ

𝑚𝑣

Substitute in the value for 𝜆. Remember that the denominator of a denominator becomes the

numerator.

This gives us:

E= ℎ𝑐𝑚𝑣

ℎ The h’s cancel out, which gives us:

E= cmv

c= velocity of light in a vacuum. Thus, it mathematically becomes:

E= mc2

Student Worksheet for Atomic Structure and Periodicity · 2017-06-18 · Student Worksheet for...

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