unit 2 problem set - web viewhow many electrons are present in the highest occupied energy level of...

Nomen: ___________________________________ R. _____________ Dies:______________IB Chemistry Year 1 HL Unit 2: Topics 3 and 13 Periodicity Problem Set

Unit 2: Periodicity Problem SetTopic 3 and 13

Multiple Choice: Please answer all multiple choice questions on the Scantron provided with you with this problem set. All multiple choice questions are worth 1 point.

1. Which species has the same configuration of electrons as a Mg2+ ion?

A. Na atom

B. F+ ion

C. Ne atom

D. O– ion

2. Which best defines electronegativity?

A. The energy required for an atom in the gaseous state to gain one electron.

B. The attraction between the nucleus and the outermost electron of an atom.

C. The attraction of an atom for a bonded pair of electrons.

D. The energy required for an atom to form a negative ion with a noble gas electron configuration.

3. Which is correct when the ionic or atomic radii are compared?

A. Ca2+ < Ca+

B. Cl– < Cl

C. Na < Na+

D. B < C

4. Which properties increase in value when descending group 1?

I. First ionization energy

II. Atomic radius

III. Reactivity with water

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

5. Which statement about a periodic trend is correct?

A. Melting points decrease from lithium to caesium.


B. Atomic radii increase from sodium to chlorine.

C. Electronegativities increase from fluorine to iodine.

D. First ionization energies increase from carbon to lead.

6. Why do the boiling points of the halogens increase down the group?

A. The molecules become more polar due to increasing electronegativities.

B. The strength of the temporary dipoles increases.

C. The bond enthalpies increase.

D. The ionization energies increase.

7. Which react with water to form acidic solutions?

I. Sodium oxide, Na2O

II. Phosphorus pentoxide, P4O10

III. Sulfur trioxide, SO3

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

8. Which of the following reacts with water to give a solution with a pH > 7?

A. Silicon dioxide

B. Sodium chloride

C. Sulfur trioxide

D. Magnesium oxide

9. Which statements are correct about the nature of Na2O, SiO2 and Cl2O?


10. Which two elements react the most vigorously with each other?

A. Potassium and iodine

B. Potassium and fluorine

C Lithium and iodine

D. Lithium and fluorine

11. Which statement is true about the values for the electronegativity of the two elements?

A. Li > K

B. Li > B

C. Br > F

D. N > O

12. Which reactions are spontaneous under standard conditions?

I. Cl2(aq) + 2NaBr(aq) → Br2(aq) + 2NaCl(aq)

II. Cl2(aq) + 2NaI(aq) → I2(aq) + 2NaCl(aq)

III. I2(aq) + 2KBr(aq) → Br2(aq) + 2KI(aq)

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

13. Which is a correct statement about the spectrochemical series?

A. It lists transition metals in order of their ability to absorb visible light.


B. It lists ligands in order of their ability to split the d orbitals of transition metals.

C. It lists the oxidation states of individual transition metals in order of their ability to absorb visible light.

D. It lists transition metals in order of their ability to transmit visible light.

14. Which statement is correct about the iron(II) ion?

A. Aqueous solutions of the ion are yellow-brown in colour.

B. It forms the [Fe(H2O)6]2+ complex ion in aqueous solution.

C. Its electron configuration is [Ar]4s23d4.

D. It can be oxidized to the iron(III) ion by carbon monoxide.

15. Which of the following form a coloured solution in water?

I. Cu(NO3)2

II. Zn(NO3)2

III. Ni(NO3)2

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

16. Which electrons are lost when copper metal forms the Cu2+ ion?

A. two s electrons

B. two d electrons

C. two p electrons

D. one s electron and one d electron

17. Which are typical properties of transition metal elements?

I. They form complex ions


II. They are good catalysts

III. They have variable oxidation states

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

18. Which substance is used as a catalyst in the industrial manufacture of ammonia?

A. V2O5

B. Pd

C. Fe

D. MnO2

19. Which substance is used as a catalyst in catalytic converters in cars?

A. Pd

B. MnO2

C. Fe

D. V2O5

20. How are cyanide ions behaving in the reaction below?

[Fe(H2O)6]2+ + 6CN–(aq) → [Fe(CN)6]4– + 6H2O(l)

A. As an oxidizing agent

B. As a reducing agent

C. As a Lewis acid

D. As a Lewis base

21. An element is in period 3 and group 15 of the periodic table. How many electrons are present in the highest occupied energy level of this element?

A. 3

B. 5

C. 13

D. 15

22. Which best describes the trends of electronegativity values within the periodic table?

A. The values increase across a period (from left to right) and decrease down a group.


B. The values increase across a period (from left to right) and increase down a group.

C. The values decrease across a period (from left to right) and decrease down a group.

D. The values decrease across a period (from left to right) and increase down a group.

23. Which is the correct trend for the elements moving from left to right across Period 3?

A. The oxides become less acidic

B. The bonding of the chlorides changes from ionic to covalent

C. The atomic radii increase

D. The melting points of the elements increases

24. The first ionization energies for three consecutive elements in the periodic table are 1251, 1521 and 419 kJ mol-1 respectively. Which elements have these values?

A. carbon, nitrogen, oxygen

B. neon, sodium, magnesium

C. sodium, magnesium, aluminium D. chlorine, argon, potassium

25. Which factors lead to an element having a high first ionization energy?

I. Completely filled outer energy level

II. Small atomic radius

III. High number of completely filled inner energy levels

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

Nomen: ___________________________________ R. _____________ Dies:______________IB Chemistry Year 1 HL Unit 2: Topics 3 and 13 Periodicity Problem Set26. Which equation represents the first ionization energy of carbon?

A. C(s) → C+(g) + e–

B. C(g) + e– → C–(g)

C. C(s) + e– → C–(g)

D. C(g) → C+(g) + e–

27. Which is a correct statement about the halogens or their ions?

A. Halide ions are all oxidising agents with the fluoride ion being the strongest

B. Bromine can oxidise iodide ions.

C. Iodine can oxidise chloride ions.

D. Fluorine is a stronger reducing agent than iodine.

28. Which are the correct products when chlorine gas reacts with water?

A. H2 and Cl2O

B. H2, O2 and HClO

C. H2, Cl2 and HClO

D. HClO + H+ + Cl-

29. Which is the correct electron configuration for the copper (I) ion ?

A. [Ar]4s13d9

B. [Ar]3d9

C. [Ar]3d10

D. [Ar]4s23d8

30. Which reaction produces a coloured substance?

A. The addition of sodium metal to water.

B. The addition of sulfur dioxide gas to water.

C. Burning sodium metal in chlorine gas.

D. The addition of chlorine gas to a solution of potassium iodide.

31. Which is a correct statement about all the elements in the same period?

A. They all contain the same number of electrons in their outer energy level

B. Their boiling points increase (going from left to right).


C. They have the same number of occupied energy levels.

D. Their atomic radii decrease (going from left to right).

32. Which support the statement that aluminium oxide is amphoteric.

I. Al2O3 can react with strong acids and bases.

II. Al2O3 dissolves in water to give a neutral solution.

III. Al2O3 can react to form a salt with sodium hydroxide and with hydrochloric

acid.

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

33. Which element is a transition metal?

A. lead, Pb

B. gallium, Ga

C. strontium, Sr

D. iron, Fe

34. What must all ligands contain?

A. An unpaired electron

B. A negative charge

C. A non-bonding pair of electrons

D. Two or more atoms or ions

15. Which species can act as ligands?

I. NH3

II. Cl-

III. SiCl4

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

Nomen: ___________________________________ R. _____________ Dies:______________IB Chemistry Year 1 HL Unit 2: Topics 3 and 13 Periodicity Problem Set36. The compounds [Cr(H2O)4Cl2]Cl and [Cr(H2O)5Cl]Cl2 are isomers. What is the oxidation state of chromium in these two compounds?

37. Which is used as a catalyst during the manufacture of sulfuric acid?

A. Ni

B. V2O5

C. MnO2

D. Fe

38. In the following reaction :

[Cu(H2O)6]2+(aq) + 4NH3(aq) → [Cu(NH3)4(H2O)2]2+(aq) + 4H2O(l)

Which are correct statements?

I. The Cu2+ ion is acting as a Lewis acid

II. [Cu(H2O)6]2+ has an octahedral shape

III. The oxidation state of copper remains unchanged

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

39. In which complex ion does the metal have an oxidation state of +2?

A. [Co(H2O)6]3+

B. [Ag(NH3)2)]+

C. [CuCl4]2–

D. [Fe(CN)6]3–

40. Which species will not be coloured?

A. Cu2SO4 B. Mn2O3


C. [Fe(H2O)6]3+ D. Pt(NH3)2Cl

Short Answer

41. The atomic and ionic radii of some elements are given in the table below:Element Atomic radius/pm Ionic Radius/pmNa 186 98Al 143 45Cl 99 181K 231 133

a. Explain why the atomic radius of aluminium is smaller than that of sodium.

[2]b. Explain why the ionic radius of aluminium is smaller than its atomic radius

but the atomic radius of chlorine is larger than its atomic radius.

[4]

c. Explain why the ionic radius of potassium is smaller than that of chlorine.

[2]d. Write equations for the first electron affinity of chlorine and the first

ionization energy of magnesium.

[2]e. Explain why the first electron affinity of chlorine is more exothermic than the

first ionization energy of bromine.


[2]f. Explain why chlorine has a higher first ionization energy than magnesium.

[2]Total 14 Points

42. Describe and explain what you will see if chlorine gas is bubbled through a solution of:

a. potassium iodide

[2]b. potassium fluoride

[1]

43. The periodic table shows the relationship between electron arrangement and the properties of elements and is a valuable tool for making predictions in chemistry.

a. Identify the property used to arrange the elements in the periodic table.

[1]b. Outline two reasons why electronegativity increases across period 3 in the periodic table and one reason why noble gases are not assigned electronegativity values.

[3]

44. The alkali metals are found in group 1 of the periodic table of elements.a. State the full electron configuration of K and K+.

[2]b. Describe what the term first ionization energy means.


[1]c. State and explain how the first ionization energies of the alkali metals vary going down Group 1.

[1]d. Explain why the ionic radius of K+ is smaller than the atomic radius of the parent atom K.

[1]e. Suggest why you should never touch an alkali metal with your fingers when working in the laboratory.

[1]45. a. Write the full electron configuration of

i. a Cu atomii. a Cu 2+ atom

[2]b. One characteristic property of transition metals is that they can form complex ions with ligands. Explain what is meant by the term ligand.

[1]c. What is the oxidation number of copper in the complex ion [CuCl4]2-?

[1]d. Explain whether CuBr is diamagnetic or paramagnetic.


[2]e. Explain why solutions containing the complex ion [Cu(H2O)6]2+ are coloured and why solutions containing the complex ion [Cu(NH3)6]+ are colorless.

[5]f. When concentrated HBr is added to copper (II) sulfate, the following reaction occurs:

[Cu(H2O)6]2+ + Br- [Cu(H2O)5Br]+ + H2OState and explain any differences in the wavelength of light absorbed by [Cu(H2O)6]2+ and [Cu(H2O)5Br]+.

[2]46. Consider the complex K4[Fe(C2O4)3].

a. Deduce the condensed electron configuration of the transition metal in this complex.

[1]b. State the geometry of the transition metal in this complex.

[1]c. Identify the nature of the bonding between the ligand and the transition metal ion in the complex.


[2]

d. State the denticity of the ethanedioato ligand.

[2]e. Draw a diagram showing the splitting of the d-sublevel. Label the orbitals involved and populate each of the orbitals with electrons.

[2]

f. Explain whether the complex is paramagnetic or diamagnetic.

[2]

47. Samples of sodium oxide and sulfur trioxide are added to separate beakers of water. Deduce the equation for each reaction and identify each as acidic, basic or neutral.

[3]48. The graph below of the first ionization energy plotted against atomic number for the first 20 elements shows periodicity.


a. State the electron configuration of Argon and explain why the Noble Gases helium, neon and argon show the highest first ionization energy.

[3]

b. Explain why the melting points of the Group 1 metals decrease down the group whereas the melting points of the Group 17 elements increase down the group.

[3]

Nomen: ___________________________________ R. _____________ Dies:______________IB Chemistry Year 1 HL Unit 2: Topics 3 and 13 Periodicity Problem SetAnswers:1. C, 2. C, 3. A, 4. C, 5. A, 6. B, 7. C, 8. D, 9. C, 10. B,11. A, 12. A, 13. B, 14. B, 15. B, 16. D, 17. D. 18. C, 19. A, 20. D.

1. B, 2. A, 3. B, 4. D, 5. A, 6. D, 7. B, 8. D, 9. C, 10. D,11. C, 12. B, 13. D, 14. C, 15. A, 16. A, 17. B. 18. D, 19. C, 20. A.

unit 2 problem set - web viewhow many electrons are present in the highest occupied energy level of...

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