Worksheets - Answers Grade 11 IB

Unit 2 Atomic StructureNo Worksheet – Mass Spectrometer Read Pgs 42 – 47, Pg 65 Q# 1 – 5Worksheet 1 – Aufbau Diagrams Read Pgs 38 – 41

Read Pgs 50 – 61 Pg 65 Q# 6 – 16Worksheet 2 – Blank Periodic TableWorksheet 3 – Energy Level DiagramsWorksheet 4 – Electron ConfigurationsWorksheet 5 – Orbital and Energy Level DiagramsWorksheet 6 – Quantum Numbers Read Pgs 291 – 299, Pg 300 Q# 1 - 4Worksheet 7 – Atomic Structure Review

Unit 3 PeriodicityWorksheet 8 – Periodic Trends Read Pgs 70 – 74, Pgs 75 – 90

Pg 91 Q#1 – 13Worksheet 9 – Alkali Metals and HalogensWorksheet 10 - PolarityNo Worksheet – d -sublevel Read Pgs 301 – 313, 316 – 326

Pg 327 Q#1 – 13

Worksheet 4 – Electron Configurations of Atoms

1) Write the full and shorthand (condensed) electron configurations for each of the following atoms.

a) phosphorus 1s22s22p63s23p3 [Ne]3s23p3

b) beryllium 1s22s2 [He]2s2

c) fluorine 1s22s22p5 [He]2s22p5

d) calcium 1s22s22p63s23p64s2 [Ar]4s2

e) zinc 1s22s22p63s23p64s23d10 [Ar]4s23d10

f) tellurium, 1s22s22p63s23p64s23d104p65s24d105p4 [Kr] 5s24d105p4

g) sodium 1s22s22p63s1 [Ne]3s1

h) nickel 1s22s22p63s23p64s23d8 [Ar]4s23d8

i) oxygen 1s22s22p4 [He]2s22p4

j) iron 1s22s22p63s23p64s23d6 [Ar]4s23d6

k) magnesium 1s22s22p63s2 [Ne]3s2

l) aluminum 1s22s22p63s23p1 [Ne]3s23p1

2) Write shorthand (condensed) electron configuration for each of the following atoms.

a) holmium [Xe]6s24f11

b) osmium [Xe]6s24f145d6

c) lead [Xe]6s24f145d106p2

d) radium [Rn]7s2

e) bohrium [Rn]7s25f146d5

3) Determine which elements have the following electron configurations:

a) 1s22s22p63s23p4 S b) 1s22s22p63s23p64s23d104p65s1 Rb

c) [Kr] 5s24d105p3 Sb d) [Xe] 6s24f145d6 Os

e) [Rn] 7s25f11 Es

4) Determine which electron configurations are not valid.

a) 1s22s22p63s23p64s24d104p5 no b) 1s22s22p63s33d5 no

c) [Ra] 7s25f8 no d) [Kr] 5s24d105p5 yes

e) [Xe] no – better to put [Kr]5s24d105p6

5) Which block of the periodic table are each of the following elements located in?

a) einsteinium f b) polonium p

c) rutherfordium d d) francium s

6) Without looking at the periodic table, identify the group number, period number, and block of an atom that has each of the following electron configurations.

a) [Ne]3s1 group 1, period 3, s block

b) [He]2s2 group 2, period 2, s block

c) [Kr]5s24d105p5 group 17, period 5, p block

7) What is the number of orbitals in each of the following subshells?

a) 2s 1 b) 4p 3 c) 3d 5 d) 1p 0

e) 4f 7 f) 2p 3 g) 2d 5 h) 6g 9

8) What is the maximum number of electrons in each of the following subshells?

a) 2s 2 b) 4p 6 c) 3d 10 d) 1p 0

e) 4f 14 f) 2p 6 g) 2d 10 h) 6g 18

Worksheet 5 – Orbital and Energy Level Diagrams

1) Identify and correct the errors in each of the following valence shell orbital diagrams: Element s orbital p orbitals

a) carbon

Correct:

b) sulfur

Correct:

c) aluminum

Correct:

2) Consider the valence level electron configurations of the following five elements:Element s orbital p orbitals

1

2

3

4

5

a) Which of the above elements are metals? 2, 3, 4 could be metals

b) Which of the above elements would form an ion with a +2 charge? 3, possibly 4

c) Which of the above elements is a noble gas? 1, possibly 3 a halogen? 5

d) Which of the above elements has the same configuration as S2- ? 1

3) Write the orbital occupied by the last electron of each of the following elements:

As W Li U O Rn V

4p 5d 2s 5f 2p 6p 3d

4) Draw an orbital diagram for each of the following.

a) a cobalt atom (Co)

1s 2s 2p 3s 3p 4s 3d

b) a sulfide ion S2–

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

c) a cadmium ion (Cd2+)

1s 2s 2p 3s 3p 4s 3d

4p 5s 4d

5) Draw a complete energy level diagram (vertical) for an atom of iron, Fe.

Worksheet 6 – Quantum Numbers

1. State the four quantum numbers and the possible values they may have.

n = 1,2,3,4,5,6,7,8 , l = 0,1,2,3 , ml = -l...+l , ms = +½ , -½

2. Name the orbitals described by the following quantum numbers

    a. n = 3, L = 0 , 3s    b. n = 3, L = 1 , 3p    c. n = 3, L = 2 , 3d    d. n = 5, L = 0 , 5s

3. Give the n and L values for the following orbitals

    a. 1s , n = 1 l = 0     b. 3s , n = 3 l = 0    c. 2p , n = 2 l = 1    d. 4d , n = 4 l = 2    e. 5f , n = 5 l = 3

4. Place the following orbitals in order of increasing energy:

    1s, 3s, 4s, 6s, 3d, 4f, 3p, 7s, 5d, 5p , 1s, 3s, 3p, 4s, 3d, 5p, 6s, 5d, 7s

5. What are the possible mL values for the following types of orbitals?

    a. s , 0    b. p , -1, 0, +1    c. d , -2, -1, 0, +1, +2    d. f , -3, -2, -1, 0, +1, +2, +3

6. How many possible orbitals are there for n =

    a. 4 , 16    b. 10 , 100

7. How many electrons can inhabit all of the n=4 orbitals? 32

8. Tabulate all of the possible orbitals (by name, i.e. 4s) for n=4 and give the three quantum numbers which define each orbital.4s n = 4, l = 0, ml = 0 4p n = 4, l = 1, ml = -1, 0, +1 4d n = 4, l = 2, ml = -2, -1, 0, +1, +2 4f n = 4, l = 3, ml = -3, -2, -1, 0, +1, +2, +3

9. Write electron configurations for the following atoms:    a. H 1s1 d. F 1s22s22p5

    b. Li 1s22s1 e. Br 1s22s22p63s23p64s23d104p5

    c. N 1s22s22p3

   

Worksheet 7 - Atomic Structure Test Review

1) Which one of the following statements regarding Rutherford’s gold foil experiment is TRUE?a) Rutherford predicted that most of the alpha particles would pass straight through the

foil because atoms are mainly empty space.b) Rutherford predicted that the alpha particles that hit negative particles would bounce

back towards the radioactive source.c) The actual experimental results led Rutherford to conclude that atoms have a central

positive core because most of the alpha particles were deflected at large angles.d) Since most of the alpha particles passed straight through the foil without deflection,

Rutherford concluded that atoms are mainly empty space.e) The most surprising thing about the experimental results was that only some of the

alpha particles were deflected at large angles.

2) In Thomson’s model of the atom:a) negative particles are embedded within a sphere of positive chargeb) atoms are tiny, indivisible spheresc) positive particles are embedded within a sphere of negative charged) there is a positive nucleus surrounded by empty space

3) Which one of the following could be the electron configuration for an element with the following Lewis diagram?

a) 1s22s1 b) 1s22s22p3

c) 1s22s22p1 d) [Ar]4s23d3

e) more than one are correct

4) The species with the following energy level diagram is:

a) Ne b) Na

c) Na+ d) K

e) Cl–

5) In the emission spectrum of hydrogen, which electronic transition would produce a line in the visible region of the electromagnetic spectrum?

a) n = 2 n = 1b) n = 3 n = 2c) n = 2 n = 3d) n = n = 1

X

6) How many unpaired electrons are in the ground state energy level diagram for an atom of sulfur?

a) 1 b) 2 c) 3 d) 4 e) 5

7) Which of the following particles has the same electron configuration as krypton?a) Ga3+ b) Ga3– c) Sn4+ d) Sn2+ e) As3–

8) Complete the following table:

Name of Element

Symbol of

Atom or Ion

Atomic Number

Mass Number

Number of

Protons

Number of

Neutrons

Number of

Electrons

Overall Charge

a beryllium Br 4 9 4 5 4 0

b fluorine F- 9 19 9 10 10 1-

c iron Fe3+ 26 56 26 30 23 3+

d selenium Se2- 34 79 34 45 36 2-

9) Write the full electron configuration for each of the following atoms:a) strontium 1s22s22p63s23p64s23d104p65s2

b) germanium 1s22s22p63s23p64s23d104p2

10) Write the shorthand electron configuration for each of the following atoms:a) silicon [Ne]3s23p2

b) molybdenum [Kr]5s24d4

c) terbium [Xe]6s24f9

d) gold [Xe]6s24f145d9

e) seaborgium [Rn]7s25f146d4

11) Draw orbital diagrams for each of the following ions (shorthand), indicate which electrons have been gained/lost:a) Cu+

4s ↑ 3d ↑↓ ↑↓

↑↓ ↑↓

↑↓

b) Pb2+

6s ↑↓

5d ↑↓ ↑↓

↑↓ ↑↓ ↑↓ 6p ↑ ↑

c) Br–

4s ↑↓

3d ↑↓ ↑↓

↑↓ ↑↓ ↑↓ 4p ↑↓ ↑↓ ↑↓

d) Sb3–

5s ↑↓

4d ↑↓ ↑↓

↑↓ ↑↓ ↑↓ 5p ↑↓ ↑↓ ↑↓

e) Ba2+

6s ↑↓

f) Sn4+

5s ↑↓

4d ↑↓ ↑↓

↑↓ ↑↓ ↑↓ 5p ↑ ↑

12) What is the maximum number of electrons in:a) n = 3 , 18 b) 3d , 10 c) 6p , 6

d) 4f , 14 e) 2s , 2 f) n = 5 , 50

g) all d orbitals of curium, Cm , 30

13) State the four quantum numbers for each of the following:a) the 31st electron of Ga , 4, 1, -1, +½

b) the 12th electron of magnesium , 3, 0, 0, -½

c) the 80th electron of mercury , 4, 2, +2, -½

d) the 54th electron of xenon , 5, 1, +1, -½

e) the 68th electron of holmium , 4, 3, 0, +½

Worksheet 8 - Periodic Trends

1) Which of the following elements has the largest atomic radius?a) beryllium b) carbon c) nitrogen d) oxygen

2) Which of the following elements has the smallest atomic radius?a) sulfur b) selenium c) oxygen d) tellurium

3) Which of the following elements has the smallest first ionization energy?a) strontium b) calcium c) barium d) magnesium

4) Which of the following elements has the largest first ionization energy?a) bromine b) potassium c) arsenic d) calcium

5) Which of the following elements has the highest electron affinity?a) chlorine b) silicon c) sodium d) phosphorus

6) Which element in the following sets should have the largest atomic radius, and why?a) boron, lithium, or fluorine b) potassium, lithium, or sodium

7) Which element in the following pairs has the higher first ionization energy?a) cesium or gold b) sulfur or phosphorusc) magnesium or aluminum d) neon or kryptone) oxygen or selenium f) barium or calcium

8) Which element in the following sets loses an electron most readily, and why?a) boron, lithium, or fluorine b) potassium, lithium, or sodium

9) List each of the following sets in order of increasing radius:a) Ne, Na+, O2–

b) Mg2+, Na+, Al3+

c) N3–, O2–, F1–

10) The ion Na+ and the atom Ne have the same electron configuration. To remove an electron from gaseous neon atoms requires 2081 kJ/mol. To remove an electron from a gaseous Na+ ion requires 4562 kJ/mol. Why are these values not the same?

11) The second ionization energy of magnesium is only about twice as great as the first ionization energy. However, the third ionization energy is about ten times as great as the first. Why does it take so much more energy to remove the third electron from magnesium?

12) The following graph shows the melting points (and boiling points) of the period 3 elements.

a) Why is there a general increase in melting point for Na, Mg, and Al?

b) Why does Si have the highest melting point?

c) Why is there a general decrease in melting point for P4, S8, and Cl2?

d) Why do the noble gases have the lowest melting point?

13) Although the first ionization energy of K is smaller than that of Ca, the second ionization energy of K is much higher than that of Ca. Why is this so?

14) Element I1 I 2 I 3 I 1 = 1st ionization energy (kJ/mol) AA 531 1087 6270 I 2 = 2nd ionization energy (kJ/mol) BB 2090 3135 4180 I 3 = 3rd ionization energy (kJ/mol) CC 523 8360 11704

a) Which of the above elements would most likely be an alkali metal?

b) Which of the above elements would most likely be a noble gas?

Worksheet 9 - Alkali Metals and Halogens

1) State whether each of the following properties increase or decrease going down the alkali metal group.

a) atomic radius

b) ionic radius

c) ionization energy

d) electronegativity

e) reactivity

2) State whether each of the following properties increase or decrease going down the halogen group.

a) atomic radius

b) ionic radius

c) ionization energy

d) electronegativity

e) reactivity

3) What is the state of matter at room temperature for each of the following?

a) F2

b) Cl2

c) Br2

d) I2

4) For each of the following, circle the correct element.

Li Si S metal

N P As smallest ionization energy

K Ca Sc largest atomic mass

S Cl Ar member of the halogen family

Al Si P greatest electron affinity

Ga Al Si largest atomic radius

V Nb Ta largest atomic number

Te I Xe member of noble gases

Si Ge Sn 4 energy levels

Li Be B member of alkali metals

As Se Br 6 valence electrons

H Li Na nonmetal

Hg Tl Pb member of transition metals

Na Mg Al electron distribution ending in s2 p1

Pb Bi Po metalloid

B C N gas at room temperature

Ca Sc Ti electron distribution ending in s2 d2

Worksheet 10 – Polarity

In each of the following problems, rank the molecules from lowest to highest polarity:

1) PF3, LiOH, SF2, NF3

2) Ni(OH)3, N2H2, CH3OH, C2H5OH

3) NO2, SeCl2, PbCl2, SO

4) PH3, PF3, NH3, NF3

5) H2O, H2S, HF, H2