Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.

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1 ELECTRONS IN ATOMS Chapter Quiz Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 1. The orbitals of a principal energy level are lower in energy than the orbitals in the next higher principal energy level. 2. The configuration 3d 4 4s 2 is more stable than the configuration 3d 5 4s In the quantum mechanical model of the atom, the probability of finding an electron within a certain volume of space surrounding the nucleus can be portrayed as a fuzzy cloud. 4. The fourth principal energy level of an atom contains 32 electrons. 5. There are five orbitals in the 4d energy level. 6. The amplitude of a wave is the distance between the crests. Fill in the word(s) that will make each statement true. 7. In the equation E = h ν, h is called The electron in a hydrogen atom has the least energy in the. 9. Einstein proposed that light is composed of particle-like quanta of energy; light quanta are known as The effect 10 occurs when light above the threshold frequency strikes a metal.

2 ELECTRONS IN ATOMS Chapter Test A A. Matching Match each description in Column B with the correct term in Column A. Write the letter of the correct description on the line. Column A 1. hertz 10. frequency 2. atomic orbital 3. spectrum 4. atomic emission spectrum 5. quantum of energy 6. amplitude 7. wavelength 8. energy level 9. Aufbau principle

3 Column B e. a range of colors seen when light passes through a prism a. the number of wave cycles that pass a given point per unit of time b. the SI unit of frequency f. Electrons enter orbitals of lowest energy first. g. a region outside the nucleus where there is high probability of finding an electron c. lines of colored light obtained by passing the light emitted by an element through a prism h. the amount of energy required to move an electron from one energy level to the next higher one d. the region around an atomic nucleus where an electron is likely to be moving i. the distance between crests of waves j. the height of a wave from the origin to the crest B. Multiple Choice Choose the best answer and write its letter on the line. 11. The fourth principal energy level has a. 4 orbitals. c. 32 orbitals. b. 16 orbitals. d. 9 orbitals. 12. If the electron configuration of an element is 1s 2 2s 2 2p 6 3s 2 3p 5, the element is a. iron. c. chlorine. b. bromine. d. phosphorus. 13. The quantum mechanical model of the atom a. is concerned with the probability of finding an electron in a certain position. b. was proposed by Neils Bohr. c. defines the exact path of an electron around the nucleus. d. has many analogies in the visible world. 14. The electron configuration of calcium is a. 1s 2 2s 2 2p 2 3s 2 3p 3 4s 2. c. 1s 2 2s 2 3s 2 3p 6 3d 8. b. 1s 2 2s 2 2p 10 3s 2 3p 4. d. 1s 2 2s 2 2p 6 3s 2 3p 6 4s The maximum number of electrons that can occupy the third principal energy level is

4 a. 18. c. 2. b. 32. d As the frequency of light increases, the wavelength a. increases. c. decreases. b. remains the same. d. approaches the speed of light. 17. The formula 2n 2 represents a. the number of sublevels in any energy level. b. the maximum number of electrons that can occupy an energy level. c. the number of orbitals in a sublevel. d. none of the above 18. In order to occupy the same orbital, two electrons must have a. the same direction of spin. c. opposite charge. b. low energy. d. opposite spin. 19. Stable electron configurations are likely to contain a. high-energy electrons. b. unfilled s orbitals. c. fewer electrons than unstable configurations. d. filled energy sublevels. 20. According to Hund s rule, when electrons occupy orbitals of equal energy, one electron enters each orbit until a. all the orbitals contain one electron, with spins parallel. b. all the orbitals contain one electron, with opposite spins. c. there are two electrons in each orbital. d. electron velocities become constant. C. Problems Solve the following problems in the space provided. Show your work. 21. Write electron configurations for these atoms, using arrows to represent electrons. Then, use the shorthand method to write the configurations. a. S b. Na

5 22. What is the frequency of radiation whose wavelength is cm? 23. Identify the elements that have the following electron configurations. a. 1s 2 2s 2 2p 6 3s 2 3p 1 a. b. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 b. c. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 7 4s 2 c. 24. Consider the elements neon, bromine, and phosphorus. Which has a. three electrons in its 3p sublevel? a. b. its highest energy level completely filled? b. c. the highest occupied energy level? c. 25. What is the maximum number of electrons that can occupy each of the first five principal energy levels? D. Essay Write a short essay for the following. 26. Explain why the 5s sublevel fills before any electrons are added to the 4d sublevel. E. Additional Matching Match each description in Column B with the correct term in Column A. Write the letter of the correct description on the line. Column A 29. photons 27. ground state 30. Heisenberg uncertainty principle 28. photoelectric effect 31. de Broglie s equation

6 32. Planck s constant Column B a. a process in which electrons are ejected by metals when certain wavelengths of light shine on them b. the lowest energy level for a given electron c. predicts that all matter exhibits wavelike motions d Js e. It is impossible to know both the velocity and the position of a particle at the same time. f. quanta of light F. True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 33. The energy of a body can change only in small discrete units. 34. The position and velocity of an electron in an atom can be determined with great certainty. 35. Above the threshold frequency, increasing the intensity of the light striking a metal increases the number of electrons ejected. 36. Electrons moving from one energy level to another emit photons. 37. The photoelectric effect will occur no matter what frequency of light strikes a metal. 38. In the Bohr model of the hydrogen atom, when the electron is in the ground state, n = The lines in the emission spectrum of hydrogen can be correlated to transitions of electrons from higher energy levels to lower energy levels. 40. The outermost s orbital of an atom contains two electrons.

7 41. According to quantum mechanics, the motions of subatomic particles may be described as wavelike. ELECTRONS IN ATOMS Chapter Test B A. Matching Match each term in Column B with the correct description in Column A. Write the letter of the correct term on the line. Column A 1. the ways in which electrons are arranged around the nuclei of atoms 10. the modern description of the electrons in atoms 2. the ejection of electrons by metals when light shines on them 3. the region around the nucleus of an atom where an electron is likely to be moving 4. An atomic orbital may describe at most two electrons. 5. the regions within which electrons have the highest probability of being found 6. When electrons occupy orbitals of equal energy, one electron enters each orbital until all the orbitals contain one electron. 7. the amount of energy required to move an electron from its present energy level to the next higher one 8. light quanta 9. Electrons enter orbitals of lowest energy first.

8 Column B g. Hund s rule a. Aufbau principle h. electron configurations b. quantum i. quantum mechanical model c. photoelectric effect j. photons d. atomic orbitals e. Pauli exclusion principle f. energy level B. Multiple Choice Choose the best answer and write its letter on the line. 11. Bohr s contribution to the development of atomic structure a. was referred to as the plum pudding model. b. was the discovery that electrons surround a dense nucleus. c. was proposed that electrons travel in circular orbits around the nucleus. d. is the quantum mechanical model. 12. What is the total number of orbitals in the third principal energy level? a. 1 c. 9 b. 4 d Core Teaching Resources

9 Name Date Class 13. What is the maximum number of electrons allowed in the third energy level? a. 2 c. 18 b. 8 d What is the maximum number of electrons that can occupy one orbital? a.1 c. 8 b.2 d The electron configuration for fluorine is a. 1s 2 2s 2 2p 3. c. 1s 2 2s 2 2p 6. b. 1s 2 2s 2 2p 5. d. 1s 2 2s 2 2p 6 3s The first three electrons that enter into p orbitals must have a. parallel spins. c. low energy levels. b. opposite spins. d. opposite charges. 17. The atom whose electron configuration is 1s 2 2s 2 2p 6 3s 2 3p 1 is a. B. c. Al. b. Na. d. Ga. 18. The configuration for the outermost energy level in Ca is a. 3s 2. c. 2s 1. b. 4s 2. d. 4s The element having the same s and p configurations for principal energy level 3 as the element F has for its principal energy level 2 is a. Na. c. P. b. Al. d. Cl. 20. The frequency and wavelength of all waves are

10 a. directly related. c. unrelated. b. inversely related. d. equal. 21. The SI unit of cycles per second is called a a. photon. c. hertz. b. quantum. d. hund. 22. Among the following groups of atoms, which have the same outer energy level configurations? a. H, He c. Mg, Al, Ca, Ga b. Li, Be, N, Ne d. N, P, As, Bi 23. The wavelength of light with a frequency of s 1 is a m. c m. b m. d m. 24. Once the electron in a hydrogen atom absorbs a quantum of energy, it a. is now in its ground state. c. has released a photon. b. is now in its excited state. d. none of the above C. Problems Solve the following problems in the space provided. Show your work. 25. Write the electron configurations for the following atoms. a. Mg b. P c. Br d. Xe

11 26. Identify the elements described below. a. Configuration = 1s 2 2s 2 2p 6 3s 2 3p 4 b. Contains a full second energy level c. Contains the first d electron d. Contains seven electrons in its fourth energy level e. Contains only two electrons in its fifth energy level f. Contains three unpaired electrons in its third energy level g. Contains five electrons in its 3d orbitals h Has its outermost electron in 7s What is the frequency of radiation whose wavelength is cm? 28. What is the energy of a photon whose frequency is s 1? h = Js

12 D. Essay Write a short essay for the following. 29. Distinguish between the Bohr model and the quantum mechanical model of an atom in terms of the positions of the electrons in an atom. E. Additional Matching Match each term in Column B with the correct description in Column A. Write the letter of the correct term on the line. Column A 30. the lowest energy level within which an electron can be found 31. the height of an electromagnetic wave from the origin to the crest 32. It is impossible to know exactly both the velocity and the position of a particle at the same time. 33. the number of electromagnetic wave cycles to pass a given point per unit of time 34. All matter exhibits wavelike motion. 35. the distance between the crests of an electromagnetic wave

13 Column B a. Heisenberg uncertainty principle b. wavelength c. ground state d. amplitude e. de Broglie s equation f. frequency F. True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 36. The energy levels in an atom can be viewed like the rungs on a ladder. 37. The electrons in an atom are arranged in concentric orbits around the nucleus. 38. The principal quantum number equals the number of sublevels within that principal energy level. 39. As many as eight electrons may occupy the same orbital. 40. In all natural phenomena, change proceeds toward the lowest possible energy state. 41. The photoelectric effect will occur only if the frequency of light striking an electron in a metal is above a certain threshold frequency.

14 42. The behavior of light can be explained in terms of waves. 43. According to the Heisenberg uncertainty principle, as the velocity of a moving particle is known with increasing accuracy, the position of that particle becomes less accurately known. 44. Quantum mechanics describes the motions of subatomic particles and atoms as waves that gain or lose energy in packages called quanta. ELECTRONS IN ATOMS Practice Problems In your notebook, solve the following problems. SECTION 5.1 MODELS OF THE ATOM 1. How many sublevels are in the following principal energy levels? a. n = 1 c. n = 3 e. n = 5 b. n = 2 d. n = 4 f. n = 6 2. How many orbitals are in the following sublevels? a. 1s sublevel d. 4f sublevel g. fifth principal energy level b. 5s sublevel e. 7s sublevel h. 6d sublevel c. 4d sublevel f. 3p sublevel 3. What are the types of sublevels and number of orbitals in the following energy levels? a. n = 1 c. n = 3 e. n = 5 b. n = 2 d. n = 4 SECTION 5.2 ELECTRON ARRANGEMENT IN ATOMS 1. Write a complete electron configuration of each atom. a. hydrogen d. barium g. krypton b. vanadium e. bromine h. arsenic

15 c. magnesium f. sulfur i. radon SECTION 5.3 PHYSICS AND THE QUANTUM MECHANICAL MODEL 1. What is the wavelength of the radiation whose frequency is s 1? In what region of the electromagnetic spectrum is this radiation? 2. An inexpensive laser that is available to the public emits light that has a wavelength of 670 nm. What are the color and frequency of the radiation? 3. What is the energy of a photon whose frequency is s 1? 4. What is the frequency of a photon whose energy is J? 5. Arrange the following types of electromagnetic radiation in order of increasing frequency. a. infrared c. visible light e. microwaves b. gamma rays d. radio waves f. ultraviolet 6. Suppose that your favorite AM radio station broadcasts at a frequency of 1600 khz. What is the wavelength in meters of the radiation from the station? THE PERIODIC TABLE Chapter Quiz Fill in the word(s) that will make each statement true. 1. In the modern periodic table, when elements are arranged according to their atomic, 1 there is a periodic repetition of properties. 2. There are 2 periods in the periodic table. 3. The elements in any 3 in the periodic table have similar physical and chemical properties. 5. For the inner transition elements, electrons are added to an f sublevel with a principal energy level that is than the period number Oxygen and sulfur, Group 6A elements, have 4 electrons in their highest occupied energy level.

16 THE PERIODIC TABLE Chapter Test A A. Matching Match each description in Column B with the correct term in Column A.Write the letter of the correct description on the line. Column A Column B 1. metal a. positively charged ion 2. halogen b. an element whose highest occupied s or p sublevels are partially filled 3. inner transition metal c. the energy needed to remove an electron from an atom in the gaseous state 4. representative element d. good conductor of heat and electric current 5. ionization energy e. an element whose highest occupied s sublevel and a nearby d sublevel contain electrons 6. alkaline earth metal f. any nonmetal in Group 7A 7. cation g. the tendency of an atom to attract electrons when the atom is in a compound 8. electronegativity h. an element in which the highest occupied s and p sublevels are filled 9. transition metal i. an element in Group 2A 10. noble gas j. an element whose highest occupied s sublevel and a nearby f sublevel contain electrons

17 B. Multiple Choice Choose the best answer and write its letter on the line. 11. In the periodic table, there is a periodic pattern in the physical and chemical properties of elements when they are arranged in order of a. increasing atomic mass. b. increasing electronegativity. c. increasing atomic radius. d. increasing atomic number. 12. Which sublevel corresponds to the transition metals in the periodic table? a. s c. d b. p d. f 13. The representative elements are a. inner transition metals. c. Group B elements. b. transition metals. d. Group A elements. 14. Which of the following elements is a metalloid? a. As c. Br b. Se d. Kr 15. When a strontium atom loses two electrons to form an Sr 2+ ion, the electrons are lost from the a. 5s orbital. c. 3d orbital. b. 5p orbital. d. 4f orbital. 16. The element iodine, I, is a a. period 5 alkali metal. c. period 5 halogen. b. period 4 halogen. d. period 5 transition metal. 17. The subatomic particle that plays the greatest role in determining the physical and chemical properties of an element is the a. proton. c. electron. b. neutron. d. photon.

18 18. Which of the following atoms would you expect to have the largest atomic radius? a. I c. Ca b. K d. Rb 19. From left to right across the second period of the periodic table, a. first ionization energy increases. c. electronegativity decreases. b. atomic radii increase. d. atomic mass decreases. 20. For which element would you expect a large jump between the first and second ionization energies? a. F c. Fe b. Ca d. Na 21. The category of elements that is characterized by the filling of f orbitals is the a. inner transition metals. c. alkali earth metals. b. alkali metals. d. transition metals. 22. Electronegativity a. generally decreases from left to right across a period. b. is the energy change that accompanies the loss of an electron from a gaseous atom. c. generally decreases from top to bottom within a group. d. is generally higher for metals than for nonmetals. 23. Atomic size generally a. increases from left to right across a period. b. decreases from top to bottom within a group. c. remains constant within a period. d. decreases from left to right across a period. 24. Of the following atoms, which one has the smallest first ionization energy? a. boron c. nitrogen b. aluminum d. silicon 25. The alkali metals do not include a. Li. c. Na. b. Ca. d. Rb.

19 C. Questions Answer the following in the space provided. 26. For the elements whose electron configurations end as follows, state the period and the group to which each element belongs. a. 5s 2 b. 4s 2 4p 4 c. 6s 2 6p Write the configurations for the highest occupied energy level for each of the following elements. a. He b. K c. Al d. Kr e. O 28. Arrange the following elements in order of decreasing ionization energy: a. Cs, Li, K b. Cl, Si, P, Ar c. Ca, Ba, Be, Sr 29. Tell whether each of the following elements is an inner transition metal, a noble gas, an alkali metal, an alkaline earth metal, or a halogen. Then give its period and group numbers. a. calcium b. cesium

20 c. fluorine d. chromium e. neon f. silver 30. Which element in each pair has the higher electronegativity value? a. Na, Mg b. Rb, I c. Cl, Br D. Essay Write a short essay for the following. 31. Why does atomic size generally increase as you move down a group of the periodic table and decrease as you move from left to right across a period? THE PERIODIC TABLE Chapter Test B A. Matching Match each term in Column B with the correct description in Column A. Write the letter of the correct term on the line. Column A 1. half the distance between the nuclei of two atoms of the same element when

21 the atoms are joined Column B 2. negatively charged ion a. electronegativity 3. the vertical columns of the periodic table 4. the nonmetallic elements of Group 7A 5. elements in which the highest occupied s and p sublevels are filled b. groups c. atomic radius d. ionization energy 6. the tendency for the atoms of an element to attract electrons when the atoms are in a compound e. periodic law 7. positively charged ion f. alkali metals 8. the energy required to remove an electron from an atom in the gaseous state g. halogens 9. the Group 1A elements h. noble gases 10. When elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties. i. anion j. cation B. Multiple Choice Choose the best answer and write its letter on the line. 11. The modern periodic table is arranged in order of increasing a. atomic mass. c. atomic size. b. atomic number. d. atomic radius. 12. The elements in Groups 1A through 7A are

22 a. alkali metals. c. transition metals. b. alkaline earth metals. d. representative elements. 13. Which of the following is true concerning the noble gases? a. Their highest occupied s and p sublevels are filled. b. They belong to Group 8A. c. They are sometimes referred to as the inert gases. d. all of the above 14. What is the number of electrons in the highest occupied energy level of an element in Group 5A? a.5 c. 8 b.3 d Among the groups of elements listed below, which have the same number of electrons in their highest occupied energy levels? a. Li, B, C, F c. K, Ca, Rb, Sr b. Na, Mg, Al, S d. N, P, As, Sb 16. An element that contains an electron in a d sublevel is a. Mg. c. Fe. b. O. d. Ne. 17. The elements that contain electrons in an f sublevel near the highest occupied energy level are referred to as a. alkali metals. c. transition metals. b. alkaline earth metals. d. inner transition metals. 18. The electron configuration of the element chlorine ends in a. 3s 2. c. 3s 2 3p 5. b. 3p 6. d. 3s 2 3p The element with 8 electrons in its 3d sublevel is a. O. c. Ar. b. Ne. d. Ni.

23 20. As you move down a group in the periodic table, atomic size generally a. increases. c. remains the same. b. decreases. d. varies randomly. 21. The largest atom from among the following is a. Li. c. Rb. b. Na. d. Fr. 22. The smallest atom from among the following is a. Na. c. Si. b. Mg. d. Cl. 23. As the number of electrons added to the same principal energy level increases, atomic size generally a. increases. c. remains the same. b. decreases. d. varies randomly. 24. Removing one electron from an atom results in the formation of an a. ion with a 1 charge. c. ion with a 7 charge. b. ion with a 1 charge. d. ion with a 7 charge. 25. Among the elements listed, which would show the largest increase between the second and third ionization energies? a. B c. Ca b. P d. Zn 26. Among the following, which element has the lowest ionization energy? a. Na c. Cs b. Cl d. I 27. Among the following, which element has the highest second ionization energy? a. Na c. Cs b. Cl d. I

24 28. Which of the following are always larger than the neutral atoms from which they are formed? a. positive ions c. cations b. negative ions d. none of the above 29. The smallest particle from among the following is a. Li. c. F. b. Li. d. F. 30. The least electronegative element from among the following is a. Na. c. Cs. b. Cl. d. S. C. Questions Answer the following in the space provided. 31. Given the outermost energy level configurations below, complete the table by providing the period number, group number, group name (if appropriate), and symbol for each element identified. Element Period No. Group No. Group Name Symbol a. 2s 2 b. 3s 2 3p 3 c. 3s 2 3p 6 d. 4s 1 e. 3d 1 4s 2 f. 4s 2 4p Arrange the following elements as described below. Li, C, K, F, Cs a. In order of decreasing atomic size

25 b. In order of increasing ionization energy c. In order of decreasing electronegativity 33. Among the following pairs of atoms, identify the larger of the two, the one with the greater first ionization energy, and the one with the lower electronegativity. Atom Larger Greater Ionization Energy Lower Electronegativity a. Li, K b. C, F c. Mg, Ca d. O, S 34. The outermost energy level configurations for the theoretical elements A E are listed below. Use the symbols A through E to answer each of the questions that follow. A = 3s 2 B = 3s 1 C = 2s 2 2p 6 D = 2s 2 2p 5 E = 2s 2 2p 3 a. Which has the lowest first ionization energy? b. Which is a noble gas? c. Which has the highest electronegativity? d. Which has the highest second ionization energy? e. Which is the largest atom? D. Essay Write a short essay for the following statement. 35. Explain why elements with high first ionization energies typically also have high electronegativity values.

26 THE PERIODIC TABLE Practice Problems In your notebook, solve the following problems. SECTION 6.1 ORGANIZING THE ELEMENTS 1. Which element listed below should have chemical properties similar to fluorine (F)? a. Li b. Si c. Br d. Ne 2. Identify each element as a metal, metalloid, or nonmetal. a. fluorine b. germanium c. zinc d. phosphorus e. lithium 3. Which of the following is not a transition metal? a. magnesium b. titanium c. chromium d. mercury 4. Name two elements that have properties similar to those of the element potassium. 5. Elements in the periodic table can be divided into three broad classes based on their general characteristics. What are these classes and how do they differ? SECTION 6.2 CLASSIFYING THE ELEMENTS 1. Use the periodic table to write the electron configuration for silicon. Explain your thinking. 2. Use the periodic table to write the electron configuration for iodine. Explain your thinking. 3. Which group of elements is characterized by an s 2 p 3 configuration? 4. Name the element that matches the following description. a. one that has 5 electrons in the third energy level

27 b. one with an electron configuration that ends in 4s 2 4p 5 c. the Group 6A element in period 4 5. Identify the elements that have electron configurations that end as follows. a. 2s 2 2p 4 b. 4s 2 c. 3d 10 4s 2 6. What is the common characteristic of the electron configurations of the elements Ne and Ar? In which group would you find them? 7. Why would you expect lithium (Li) and sulfur (S) to have different chemical and physical properties? 8. What characterizes the electron configurations of transition metals such as silver (Ag) and iron (Fe)? SECTION 6.3 PERIODIC TRENDS 1. Explain why a magnesium atom is smaller than atoms of both sodium and calcium. 2. Predict the size of the astatine (At) atom compared to that of tellurium (Te). Explain your prediction. 3. Would you expect a Cl ion to be larger or smaller than an Mg 2+ ion? Explain. 4. Which effect on atomic size is more significant, an increase in nuclear charge across a period or an increase in occupied energy levels within a group? Explain. 5. Explain why the sulfide ion (S 2 ) is larger than the chloride ion (Cl ). 6. Compare the first ionization energy of sodium to that of potassium. 7. Compare the first ionization energy lithium to that of beryllium. 8. Is the electro negativity of barium larger or smaller than that of strontium? Explain. 9. What is the most likely ion for magnesium to form? Explain. 10. Arrange oxygen, fluorine, and sulfur in order of increasing electro negativity.