Chem. workbook for G.11 on unit 2 PDF

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CHEMISTRY WORKBOOK FOR GRADE 11 ON UNIT TWO DIRECTIONS: Each of the following questions is followed by four possible alternatives. Choose the best answer and Circle the letter of your choice. You may refer to the information given below when you work on some of the questions. PHYSCAL CONSTANTS a) Rydberg constant (RH) = 2.18 x 10-18J b) Avogadro’s number = 6.023 x1023 mol-1 c) Plank’s constant, h = 6.626 x 10-34 Js-1 d) Speed of light, c = 2.9979 x 108 ms-1 = 3.0 x 108 m/s ATOMIC NUMBERS (Z) AND ATOMIC WEIGHTS (A) Element Z A

H 1

He 2

Li 3

B 5

C 6

N 7

O 8

F 9

Ne 10

Na 11

Mg 12

1.0

4.0

6.9

10.8

12.0

14.0

16.0

19.0

20.2

22.98 24.30

S 16

Cl 17

Ca 20

32.1

35.5

40.1

Element

Cr

Mn

Fe

Co

Ni

Cu

Zn

Ag

Cd

Au

Hg

Z

24

25

26

27

28

29

30

47

48

79

80

A

51.996

54.94

55.85

58.93

58.70

63.55

65.37

107.87

112.47

196.97

200.59

EUEE-Chemistry from Grade 11 Unit 2 (Atomic structure and Periodic table) EUEE-Chemistry 2004 E.C/2012 G.C 1. The compound CuCl emits blue light having a wavelength of 450nm when heated at about 200°C. What is the increment in energy (quantum) that is emitted at 450nm? A. 2.25 x 10-19J C. 8.20 x 10-19J B. 4.41 x 10-19J D. 16.20 x 10-19J 2. What is the difference between chlorine-35 and chlorine-37? A. Chlorine-37 has two more protons than chlorine-35 B. Chlorine-37 has two more neutrons than chlorine-35 C. Chlorine-37 has two more electrons than chlorine-35 D. Chlorine-37 has two more protons and more neutron than chlorine-35 3. Which one of the following electromagnetic radiations has the shortest wavelength? A. X – rays B. UV rays C. gamma rays D. microwaves 4. Which of the following quantum number/s determine the energy of an electron in a hydrogen atom? A. n B. n and 1 C. n, 1 and m D. n,1,m and s 5. Which of the following electron transitions requires the smallest energy to be absorbed by the hydrogen atom? A. from n = 1 to n = 2 C. from n = 3 to n = 4 B. from n = 2 to n = 3 D. from n = 4 to n = 5 6. For an electron that has quantum numbers n = 4 and m = 0, which of the following is true? A. It must have the quantum number n = 0 B. It must have the quantum number l = 0 C. It must have the quantum number ms = +1/2 D. It may have the quantum number  = 0,1,2,3 7. Which group of elements is characterized with ns2np2 outer – electron configuration? A. Group IIA B. Group IVA C. Group IVB D. Group IIIB ACADEMIC YEAR: 2013 E.C

[Solomon A.]

Page 1

CHEMISTRY WORKBOOK FOR GRADE 11 ON UNIT TWO 8. For elements in the left-most column of the periodic table, properties that have increasing values as the atomic number increases include which of the following? I. Ionization energy II. Atomic radius III. Atomic mass A. III only B. I, II, and III C. I and II only D. II and III only 9. What did Rutherford’s alpha particle experiment show? A. Electrons have a negative charge B. A proton is a hydrogen atom without electron C. Electrons circle the nucleus of an atom in orbits D. Most of the mass and all of the positive charge of an atom’s found in a tiny nucleus EUEE-Chemistry 2005 E.C/2013 G.C 1. Which of the following statements is TRUE? A. Ultraviolet light has longer wavelength than visible light B. The energy of radiation decreases as the wavelength decreases C. The frequency of radiation increases as the wavelength decreases D. Wave number of an electromagnetic radiation increases as wavelength increases 2. Which one of the following groups in the periodic table has paramagnetic atoms? A. Group zero B. Group IIA C. Group IIB D. Group IVA 3. Which of the following quantum number(s) is (are) related to the size and energy of an electron in a hydrogen atom? A. n B. n, l C. n, l, ml D. n, l, ml, ms 4. Which of the following represents the general configuration of the transition elements? A. ns2 np6 B. ns(n-l)d C. ns(n-2)f D. ns2np6(n-1)d10 5. An electron has a spin quantum number, s = +1/2 and a magnetic quantum number, m1 = +1. In which of the following orbital will it NOT be present? A. s-orbital B. p-orbital C. d-orbital D. f-orbital 6. What is the wavelength associated with an electron of mass, m= 9.11 x 10 -28g, travelling at 40% of the velocity of light? A. 6.06 x 10-15m C. 6.06 x 10-12m B. 2.42 x 10-15m D. 2.42 x 10-11m 7. What sizes of particles and velocities can one consider quantum effect? A. Particles with very large mass and large velocities B. Particles with large mass and small velocities C. Particles with very small mass and large velocities D. Particles with small mass and small velocities 8. The quantum numbers listed below are meant for four different electrons in an atom. I. n = 4, l = 0, ml = 0, ms = + ⁄ II. n = 3, l = 1, ml = 1, ms = + ⁄ IV. n = 4, l = 1, ml = 0, ms = + ⁄ III. n = 4, l = 2, ml = 0, ms = + ⁄ When these sets of quantum numbers are arranged in order to increasing energy, one may set: A. I < III < II < IV C. II < I < III < IV B. I < II < III < IV D. IV < III < II < I EUEE-Chemistry 2006 E.C/2014 G.C 1. Which electron transition in a hydrogen atom releases the largest energy? A. n = 2  n = 1 B. n = 4  n = 2 C. n = 6  n = 3 D. n = 7  n = 6 ACADEMIC YEAR: 2013 E.C

[Solomon A.]

Page 2

CHEMISTRY WORKBOOK FOR GRADE 11 ON UNIT TWO 2. What is the ration of the energy of a photon of 300nm wavelength radiation to that of 600nm radiation? A. 1:2 B. 1:1 C. 2:1 D. 3:1 3. Which of the following particles contains more electrons than neutrons? II .1735 Cl  III.1939 K  I .11 H 4.

5.

6. 7.

8.

9.

A. I only B. II only C. I and II only D. II and III only Which one of the following atoms in its ground state has the greatest number of unpaired electrons? A. 13Al B. 14Si C. 15P D. 16S What is the ionization energy of an iron atom if it requires a radiation of 276nm to completely remove its outer most electrons in the gaseous state? (Plank’s constant, h = 6.626 x 10-34Js, speed of light, c = 3 x 108 ms-1) A. 7.21 x 10-19J B. 7.21 x 10-19kJ C. 7.21 x 1019J D. 7.21 x 1019kJ How many 3d electrons are present in the ground state of chromium atom? B. 4 B. 5 C. 6 D. 10 Which of the electron configurations describes the ground state electron configuration of Cl-? A. 1s22s22p63s23p6 C. 1s22s22p63p1 2 2 6 1 B. 1s 2s 2p 3s D. 1s22s22p63s23px23py1 In which region of the periodic table would the element with the electronic structure below be located? 1s22s22p63s23p63d104s24p65s2 A. Group VI B. Noble gases C. s block D. d block Which set of quantum numbers (n, l, ml, ms) is NOT possible? A. 1, 0, 0, ½ B. 1, 1, 0, ½ C. 1, 0, 0, -1/2 D. 2, 1, -1, ½

EUEE-Chemistry 2007 E.C/2015 G.C 1. Of the three types of radioactivity characterized by Rutherford. Which of the following are particles? A.  - rays C.  – rays and  – rays B.  - rays D.  - rays,  - rays, and  – rays 2. Which one of the following represents an acceptable possible set of quantum numbers (in the order n, l, m1, ms) for an electron in an atom? A. 2, 1, 0, 0 C. 2, 1, -1, 1/2 B. 2, 0, 2, +1/2 D. 2, 0, 1, -1/2 3. How many orbitals are there in an atom with n = 4? A. 2 B. 8 C. 16 D. 25 4. Consider the three electromagnetic waves shown below.

Which of the electromagnetic waves has the highest frequency? A. 1 B. 2 C. 3 ACADEMIC YEAR: 2013 E.C

[Solomon A.]

D. 4 Page 3

CHEMISTRY WORKBOOK FOR GRADE 11 ON UNIT TWO 5. The wave number of an electromagnetic radiation is 1 x 105cm-1. The frequency of the radiation would be A. 3 x 108 s-1 B. 3 x 106 s-1 C. 3 x 1010 s -1 D. 3 x 1015 s -1 6. The maximum number of electrons in p-orbital with n = 6, ml = 0 is A. 2 B. 6 C. 16 D. 14 7. Which of the following transitions will emit maximum energy in the hydrogen atom? A. n = 4  n = 3 C. n = 2  n = 1 B. n = 4  n = 2 D. n = 3  n = 2 8. Which of the following statements is true? A. All forms of electromagnetic radiation are visible B. Radio waves have shorter wavelengths than visible light C. Ultraviolet light has longer wavelengths than visible light D. The frequency of radiation increases as the wavelength decreases 9. Which of the following diagram describes the electron density in the dxy orbital?

EUEE-Chemistry 2008 E.C/2016 G.C 1. Which of the following are NOT electromagnetic waves? A. Infrared waves C. Radio waves B. Gamma waves D. sound waves 2. What is the distance that a radio wave will travel in 0.250s? A. 1.2 x 107m B. 12 x 107m C. 7.5 x 107m D. 5.6 x 107m 3. What values of l are permitted for an electron with n = 4? A. 1, 2, 3 B. 1, 2, 3, 4 C. 0, 1, 2, 3, 4 D. 0, 1, 2, 3 4. Which of the following electrons, identified only by their n and l quantum numbers have the highest energy? n = 3, 1 = 0; n = 4, 1 = 1; n = 3, 1 = 2; n = 4, 1 = 2 A. n = 3, 1 = 2 B. n = 4, 1 = 1 C. n = 4, 1 = 2 D. n = 3, 1 = 0 5. What is the maximum number of unpaired electrons in a d subshell? A. 2 B. 5 C. 3 D. 4 6. The following energy level diagram represents the outermost shell of what ground state element?

3p

3s

A. B B. He C. Al D. Be 7. Which of the following types of rays combine to form atoms of helium? A. Gamma   rays

B. beta   rays

ACADEMIC YEAR: 2013 E.C

C. alpha   rays [Solomon A.]

D. X-rays Page 4

CHEMISTRY WORKBOOK FOR GRADE 11 ON UNIT TWO 8. What is the relationship between frequency (v), wavelength   and the speed of light (c)?  hc v A.  = c B. vc = h  C.  D. c = v  9. What is the magnitude of quantum energy and the frequency for an object whose wavelength is 0.6 x 10-6 m? A. 3.31 x 10-19J, 5x 1014S-1 C. 1.99 x 10-25J, 3.98 x 10-4S-1 -40 -15 -1 B. 3.98 x 10 J, 2 x 10 S D. 9.94 x 10-12J, 1.99 x 10-25S-1 10. What new concept did Bohr adapt and use to formulate his model of the atom? A. Electromagnetic theory developed by Maxwell B. The quantum concept developed by Planck C. Photoelectric theory developed by Thomson D. Neutron theory developed by Chadwick EUEE-Chemistry 2009 E.C/2017 G.C 1. What is the ground state electron configuration of Cu2+? A. [Ar]4s13d8 B. [Ar]4s23d7 C. [Ar]4s13d10 D. [Ar]3d9 2. Which of the following is the correct order for electron filling in orbitals? A. 3s, 3p, 4s, 3d B. 2p, 3s, 3p, 3d C. 3p, 4s, 3d, 5s D. 4s, 3d, 4p, 4d 3. The normal human eye responds to visible light of wave length ranging from about 390 to 710nm. What is the frequency range of the human eye? A. 7.7x1014s-1 to 4.2x1014s-1 C. 1.3x10-15s-1 to 2.4x10-15s-1 C. 4.2x1014s-1 to 7.7x1014s-1 D. 2.4x10-15s-1 to 7.7x10-15s-1 4. How many different types of orbitals are in the third energy level? A. 2 B. 3 C. 6 D. 7 5. The Heisenberg uncertainty principle states that: A. Two atoms of the same element must have the same number of protons B. No two electrons in the same atom can have the same set of four quantum numbers C. It is impossible to determine both positions and momentum of an electron simultaneously D. Electrons of atoms in ground state enter energetically equivalent set of orbitals singly before they pair up in any orbitals of the set 6. Which of the following transition will have minimum wavelength? A. n4 → n1 B. n2 → n1 C. n4 → n2 D. n3 → n1 7. What is the energy associated with one photon of a microwave radiation having a frequency of 2.45x109s-1? A. 1.62x1024J B. 2.45x109J C. 2.45x10-9J D. 1.62x10-24J 8. What is the frequency of radiation (in Hz) from an atom if its wavelength is 1.0x10 -9nm? A. 3.3x10-27 B. 3.0x1017 C. 3.0x108 D. 3.0x1026 9. Which of the following particle was discovered by the cathode ray experiment? A. electron B. neutron C. nucleus D. proton EUEE-Chemistry 2010 E.C/2018 G.C 1. Who used the cathode ray tube to discover the electron and determine its charge to mass ratio? A. J.J Thomson C. James Chadwick B. Robert A. Millikan D. Ernest Rutherford ACADEMIC YEAR: 2013 E.C

[Solomon A.]

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CHEMISTRY WORKBOOK FOR GRADE 11 ON UNIT TWO 2. What is the maximum number of electrons in an atom that can have the principal quantum number, n =4? A. 34 B. 32 C. 18 D. 8 3. Which quantum number is used to determine subshells? A. Azimuthal quantum number C. Magnetic quantum number B. Principal quantum number D. Spin quantum number 4. The maximum kinetic energy of a photoelectric emitted from a metal is 1.03x10 -19J when light that has a 656nm wavelength shines on the surface. What is the threshold frequency of this metal? 5. Which of the following is fundamentally different from the others? A. Microwaves B. Radio waves C. Light waves D. Sound waves 6. Which of the following equations express de Broglie’s hypothesis? A. υ = ⁄ B. λ = h/mv C. ∆E = hc/λ D. ∆E = c/λ 7. Which of the following statements about oxygen and fluorine is NOT correct? A. O and F have the same number of core electrons B. O has a smaller electron affinity than F C. O has smaller atomic radius than F D. O2- has a larger ionic radius than F8. What would be the wavelength of a radio wave having a frequency of 3MHz? A. 300m B. 100m C. 100nm D. 300nm 9. Which of the following correctly lists electromagnetic waves in order from shortest to longest wavelengths? A. Gamma rays, infrared, ultraviolet, microwaves B. Microwaves, ultraviolet, visible light, gamma rays C. Radio waves, infrared, gamma rays, ultraviolet D. Gamma rays, ultraviolet, infrared, microwaves EUEE-Chemistry 2011 E.C/2019 G.C 1. What aspects of the modern view of atomic structure was proved by Rutherford’s gold foil experiment? A. The existence of nucleus C. The charge on an α-particle B. The charge on electron D. The existence of an electron 2. In the electromagnetic spectrum with wavelengths shown (in micrometers, ηm), which bracketed section of the spectrum represents visible light?

A. O B. X C. Y D. Z 3. Which of the orbitals in the figure below has/have an angular momentum quantum number of l = 2?

A. I

B. I and II

ACADEMIC YEAR: 2013 E.C

C. II [Solomon A.]

D. I and IV Page 6

CHEMISTRY WORKBOOK FOR GRADE 11 ON UNIT TWO 4. Which of the following elements has the highest fifth ionization energy (IE 5)? A. Al B. Si C. P D. S 5. Consider the following two possibilities for electron transfer in a hydrogen atom, given below: First: The electrons drops from the Bohr orbit n = 3 to the orbit n = 2, followed by the transition from n = 2 to n = 1. Second: The electron drops from the Bohr orbit n = 3 directly to the orbit n = 1 Which of the following is correct about the energy changes of these transitions? A. The sum of the energies for the first transition is less than the energy transition of the second B. The sum of the energies for the first transition is equal to the energy transition of the second C. The sum of the energies for the first transition is greater than the energy transition of the second D. The energies of transition of the first and the energy transition of the second can’t be compared 6. The energy of an electron in the first Bohr orbit of hydrogen atom is -13.6 eV. The possible value of the exited state for electron in Bohr orbit of hydrogen is _____________? A. -1.51eV B. -6.8eV C. -4.21eV D. +6.8eV 7. The sublevel that can be occupied by a maximum of 10 electrons is identified by the letter ________ A. d B. f C. p D. s 8. Which of the following is NOT true about the photoelectric effect? A. Most metals require UV light to emit electrons B. A bright light causes more electrons to emitted than a weak light C. Higher frequency of light emits electrons with higher kinetic energy D. A bright light causes less electrons to be emitted than a weak light EUEE-Chemistry 2012/13 E.C/2020/21 G.C 1. Which of the following states the law of definite proportions? A. Every compound always contains the same elements in the same proportion by weight B. The total mass in the universe is always constant C. The mass of the products in a chemical reaction must be equal to the mass of the reactants D. Chemical compounds are formed when atoms combine in whole number ratios 2. An element X has two naturally occurring isotopes. X (10.013 amu) and X (11.01 amu). The first accounts for 19.9% of the total and the second accounts for the remaining 80.1%. What is the average atomic mass of the element X? A. 10.812 B. 10.211 C. 10.512 D. 10.125 3. What did J.J. Thomson contribute with his experiments in cathode ray tubes in understanding the atomic structure of the atom? A. Cathode rays and electric charge were combined together, and not separate entities B. Cathode rays were actually electrons C. The electric charge deposited was negative D. Cathode rays and electric charge were separate entities and not combined together 4. What are isotopes? Isotopes are atoms with the same number of protons but different number of A. electrons B. protons C. ions D. neutrons 5. How much energy would be released as an electron is moved from the n = 4 to the n = 3 energy level? (RH = 2.18 x 10-18J). A. 1.050 x 10-19 J C. 2.043 x 10-18 J B. 1.938 x 10-19 J D. 3.981 x 10-18 J ACADEMIC YEAR: 2013 E.C

[Solomon A.]

Page 7

CHEMISTRY WORKBOOK FOR GRADE 11 ON UNIT TWO 6. Which statement is CORRECT for the emission spectrum of the hydrogen atom? A. The lines are produced when electrons move from second to fourth B. The line in the visible region involve electron transitions into the energy level closest to the nucleus C. The lines are produced when electrons move from lower to higher energy levels D. The line corresponding to the greatest emission of energy is in the ultraviolet region 7. Which set of quantum numbers uniquely defines one of the electrons in an atomic orbital with n = 2 and l = 0? A. n = 2, l = 0, ml = 0, ms =+1 C. n = 2, l = 0, ml = 0, ms =+1/2 B. n = 2, l = 0, ml = 1, ms =+1 D. n = 2, l = 0, ml = 1, ms =+1/2 8. What is Pauli Exclusion Principle? The Pauli Exclusion Principle states that A. all electrons in an atom are in the same energy state B. no two electrons in an atom can have the same set of the four quantum numbers C. two electrons in an atom can have the same set of the four quantum numbers D. an orbital can hold a maximum of two electrons with the same quantum number ms 9. Which of the following is the CORRECT relationship between the given parameter and the property of an EMR? A. The higher the value of the wave length of an EMR, the greater is its frequency B. The lower the value of the frequency of an EMR, the higher is the energy of an EMR C. The higher the value of the wave length of an EMR, the greater is its energy D. The lower the frequency of an EMR, the higher is its wave length

Additional Questions on Unit Two 1. The mass-to-charge ratio of the proton is found to be 1.044×10-8 kg/C. The charge on the proton is 1.602×10-19 C. Calculate the mass of the proton. 2. An oil-drop experiment results in the following charges on oil droplets: 6.4×10-19 C, 3.2×10-19C and 4.8×10-19C. What value for the electronic charge can be deduced from this experiment? 3. What is a cathode ray? How was the nature of cathode rays determined? What are the characters of cathode ray? 4. Describe J. J. Thomson’s experiment that determined the mass-to-charge ratio of the electron. 5. Describe Millikan’s oil-drop experiment. How did Millikan determine the charge on an electron? 6. What is radioactivity? How was it discovered? 7. How do gamma rays differ from X-rays? How are the two kinds of rays similar? 8. How did the discovery of radioactivity cause Dalton’s atomic theory to be modified? 9. What is an atom? 10. Does a...