AP Chemistry Test (Chapter 7) Multiple Choice (50%) 1) Which electron would be most likely to absorb red light? A) n = 2 n = 3 B) n = 1 n = 7 C) n = 3 n = 2 D) n = 7 n = 1 2) Which statement about electromagnetic radiation is true?

A) The frequency of radio waves is greater than the frequency of infrared waves. B) λ is inversely proportional to frequency. C) Photons of ultraviolet waves have more energy than photons of X-rays. D) The λ of violet light is longer than the λ of yellow light. E) The velocity of all electromagnetic waves is constant. 3) Which element is characterized by 5 valence electrons in the 4th energy level? A) Sb B) Br C) As D) Bi E) None of these 4) Which element is characterized by the ending electron configuration 5d4 ? A) Tc B) W C) Re D) Zr E) None of these 5) What is the ending electron configuration for Pb? A) 6p2 B) 5p2 C) 2p6 D) 2p5 E) None of these 6) What would be the outer electron configuration of the boron family/group? A) ns2np2 B) ns2np5 C) ns2np1 D) ns2np4 E) ns2nd5np6

7) How many electrons are possible for one d-orbital? A) 6 B) 0 C) 5 D) 10 E) 2 8) How many spatial orientations are possible for a d-orbital? A) 4 B) 5 C) 2 D) 0 E) 10

9) If the following set of quantum numbers represents the “last” electron added to complete the ground state electron configuration of an element according to the Aufbau Principle, which one of the following could be the element?

n = 3, l = 2, ml = -2, ms = + ½

A) Mg B) Al C) Ga D) Ni E) Pd 10) Which quantum number is not possible for the f-orbitals? A) n = 4 B) l = 2 C) ml = -2 D) n = 5 E) ml = +3 11) Which one illustrates the concept of ionization energy? A) X + e- X– B) X+ + e– X C) X X+ + e– D) X– X+ + e– E) X X– + e–

12) Within the same period of elements, which one would have the greatest electron affinity? A) ns2np2 B) ns2nd10 C) ns2 D) ns2np5 E) ns2np1 13) An element has the following valence Aufbau diagram. Which one would be its oxidation

number in simple ionic compounds?

_ _ ___ ns np np np

A) +3 B) –3 C) +1 D) –1 14) Which one is false about the absorption spectrum of an element? A) The spectrum contains predominately ROYGBIV. B) White light passes through a sample of the gaseous element. C) The spectrum has dark bands where the element absorbs certain frequencies of light. D) The wavelengths of light the element absorbs are equivalent to the wavelengths of light it emits. E) The spectrum contains predominately sharp bands of light.

15) Which set of quantum numbers is not possible? A) n = 5, l = 0, ml = 0, ms = + ½ B) n = 6, l = 2, ml = +1, ms = + ½ C) n = 4, l = 2, ml = -1, ms = - ½ D) n = 6, l = 3, ml = +2, ms = + ½ E) n = 5, l = 3, ml = -3, ms = + ½

16) Which Aufbau diagram is incorrect?

A) _ ___ 1s 2s 2px 2py 2pz

B)

1s 2s 2px 2py 2pz

C) 1s 2s 2px 2py 2pz

D) _ _

1s 2s 2px 2py 2pz 17) Which orbital fills after 5s2? A) 6p6 B) 3d10 C) 4f14 D) 4d10 E) 5p6 18) Which one is true about a photon? A) It is so small that its particle nature dominates its wave nature. B) It is so small that its wave nature dominates its particle nature. C) It is so small that its wave nature can be ignored. D) It is so large that its wave nature can be ignored. 19) Which one of the following pairs contains isoelectronic species? A) O2- and Al3+ B) Ca2+ and Ca C) S2- and O2- D) K+ and O2-

E) Rb+ and K+

20) Which one is false about the atomic emission spectrum of an element? A) It is a distinct method of identifying an element from its emitted light. B) It is line spectrum of light. C) Electrons absorb white light to move from a lower energy cloud to a higher energy cloud. D) Electrons emit light as they move from a higher energy cloud back to a lower energy cloud. E) The Aurora Borealis is an example of the emission spectra of nitrogen and oxygen. 21) Which one includes all of the species that have the electronic configuration, 1s22s22p63s23p64s23d104p6 ? A) Mg2+ and Ca2+ B) Se2- and Y3+

C) Br - and K+ D) As3+ and V3+ E) Rb+ and Zr+

22) Which one is true about an atom of aluminum? A) 1st IE < 2nd IE <<<<<<<<<<<<<< 3rd IE B) 1st IE > 2nd IE > 3rd IE >>>>>>>>>> 4th IE C) 1st IE > 2nd IE >>>>>>>>>>>>>> 3rd IE D) 1st IE < 2nd IE < 3rd IE <<<<<<<<<< 4th IE E) 1st IE < 2nd IE < 3rd IE < 4th IE <<<<<<<<<<<<<<<< 5th IE 23) Please arrange the following elements in order of increasing atomic radii. Zn, Se, S, Ti A) S<Se<Ti<Zn B) Se<S<Ti<Zn C) Se<S<Zn<Ti D) Ti<Zn<Se<S E) S<Se<Zn<Ti 24) Please arrange these elements in order of decreasing first ionization energy.

Cs, Ar, Cl, Mg A) Cl, Ar, Mg, Cs B) Ar, Mg, Cl, Cs C) Ar, Cs, Mg, Cl D) Ar, Cl, Mg, Cs E) Mg, Cs, Cl, Ar

25) Please arrange the following elements in order of increasing electron affinity. Cr, N, Y, P A) N, P, Cr, Y B) P, N, Y, Cr C) Y, Cr, P, N D) Cr, P, Y, N E) Cr, Y, P, N Problems and Free Response (60%) PLEASE SHOW ALL YOUR WORK FOR ANY CREDIT! 1) 5.00 m 0.887 m 2.48 s A) ________________ What is the velocity? B) ________________ What is the amplitude? C) ________________ What is the period? D) ________________ What is the wavelength? E) ________________ What is the frequency?

2) Explain each of the following observations using principles of atomic structure and/or bonding.

a) The ionic radius of Sr2+ is smaller than that of Se2-.

b) The ionic radius of N3¯ is larger than that of O2¯.

c) A calcium atom is larger than a zinc atom.

d) Boron has a lower first-ionization energy than beryllium.

3) An electron has a mass of 9.11 X 10-31 kg. An electron emits photons of green light when it transitions from n = 5 to n = 2. The wavelength of green light is 515 nm.

A) What is the energy of a photon of green light? B) What is the frequency of green light? C) What is the energy of the electron at each energy level? D) Indicate whether the atom emits energy or whether it absorbs energy during the transition. Justify your answer. E) If the electron is moving at a velocity of 2.0 X 108 m/s, what is its wavelength? 4) A) The values of the first three ionization energies (I1,I2, I3) for magnesium and argon are as follows: I1 I2 I3 (kJ/mole) Mg 735 1443 7730 Ar 1525 2665 3945

In terms of these configurations, explain why the values of the first and second ionization energies of Mg are significantly lower than the values for Ar, whereas the third ionization energy of Mg is much larger than the third ionization energy of Ar.

B) Element Q has the following first three ionization energies:

I1 I2 I3 (kJ/mole) Q 496 4568 6920

What is the formula for the most likely compound of element Q with chlorine? Explain the choice of formula on the basis of the ionization energies.

5) The emission spectrum of hydrogen consists of several series of sharp emission lines in the ultraviolet (Lyman series), in the visible (Balmer series), and in the infrared (Paschen series, Brackett series, etc.) regions of the spectrum.

A) What feature of the electronic energies of the hydrogen atom explains why the

emission spectrum consists of discrete wavelengths rather than a continuum of wavelengths?

B) Account for the existence of several series of lines in the spectrum. What quantity

distinguishes one series of lines from another? 6) A) Discuss some differences in physical and chemical properties of metals and nonmetals.

B) What characteristic of the electronic configurations of atoms distinguishes metals from nonmetals? C) On the basis of this characteristic, explain why there are many more metals than nonmetals.

AP Chemistry Test (Chapter 7) Name_________________________________ Multiple Choice (50%) 1) _____ 16) _____

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Problems and Free Response (60%) 1) Please use only the front side of each piece of paper. 2) Please number your problems clearly and consecutively. 3) Please staple your problems to the back of this page in numerical order. 4) Please write on the paper in the conventional manner. 5) Please do not make a separate list of answers. Record your answer at the end of the work

supporting your answer. 6) Please circle/box your answer to any problems.