CHEMISTRY:MOLECULAR NATURE (LL)W/ACCESS
7th Edition
ISBN: 9781119497325
Author: JESPERSEN
Publisher: WILEY
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Chapter 7, Problem 66RQ
Going from left to right in the periodic table, why are the size changes among the
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The periodic table is the most important organizing principle in chemistry. There is a regular progression in the periodic table that reflects a similar regularity in the structures and properties of the different elements. If you know the properties of any one element in a group, you can make a good guess at the properties
of every other element in the same group and even the elements in neighboring groups. Familiarizing yourself with the structure and arrangement of the periodic table early on will help you later on in chemistry.
Part A
Classify the following elements as main group elements, transition metals, or inner transition metals.
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Ca Sn Fm Pd Zn S
Transition metals
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15.
(a)
b)
Identify the element that is described by the following information. Refer to a
periodic table if necessary.
It is a group 14 (III A) metalloid in the 3rd period.
It is a group 15 (VA) metalloid in the 5th period.
It is the other metalloid in group 15 (VA).
d)
It is a halogen that exists in the liquid state at room temperature.
16.
What is the relationship between electron arrangement and the organization of
elements in the periodic table?
6 The elements of the Periodic Table are created by a variety of processes discussed in the Astronomy course (nucleosynthesis). Describe several of the processes that are responsible for the formation of
chemical elements in different regions of the Periodic Table.
Chapter 7 Solutions
CHEMISTRY:MOLECULAR NATURE (LL)W/ACCESS
Ch. 7 - Practice Exercise 7.1
Helium derives its name from...Ch. 7 - Practice Exercise 7.2
Radio station KRED in...Ch. 7 - Calculate the wavelength in micrometers, m, of...Ch. 7 - Practice Exercise 7.4
Calculate the wavelength in...Ch. 7 - What is the energy of the radiation emitted when...Ch. 7 - Practice Exercise 7.6
If the energy of light...Ch. 7 - Calculate the energy of an electron in its lowest...Ch. 7 - Practice Exercise 7.8
If an electron moves from a...Ch. 7 - Practice Exercise 7.9
What are the values of n and...Ch. 7 - What subshells would be found in the shells with...
Ch. 7 - Without looking at the tables in the text, how...Ch. 7 - Prob. 12PECh. 7 - Practice Exercise 7.13
Draw orbital diagrams for...Ch. 7 - Practice Exercise 7.14
Use Figure 7.18 to predict...Ch. 7 - Can an dement with an even atomic number be...Ch. 7 - Practice Exercise 7.16
Use orbital diagrams to...Ch. 7 - Practice Exercise 7.17
Use the periodic table to...Ch. 7 - Use the periodic table to predict the electron...Ch. 7 - Practice Exercise 7.19
Write shorthand...Ch. 7 - Write shorthand configurations and abbreviated...Ch. 7 - Practice Exercise 7.21
Give an example of a...Ch. 7 - Prob. 22PECh. 7 - Prob. 23PECh. 7 - Practice Exercise 7.24
Use the periodic table to...Ch. 7 - Use the periodic table to select the atom with the...Ch. 7 - Prob. 26PECh. 7 - In general terms, why do we call light...Ch. 7 - In general, what does the term frequency imply?...Ch. 7 - What is meant by the term wavelength of light?...Ch. 7 - 7.4 Sketch a picture of a wave and label its...Ch. 7 - Which property of light waves is a measure of the...Ch. 7 - Arrange the following regions of the...Ch. 7 - 7.7 What wavelength range is covered by the...Ch. 7 - Arrange the following colors of visible light in...Ch. 7 - What is the equation that relates the wavelength...Ch. 7 - How is the frequency of a particular type of...Ch. 7 - 7.11 What is a photon?
Ch. 7 - Show that the energy of a photon is given by the...Ch. 7 - Examine each of the following pairs and state...Ch. 7 - What is a quantum of energy?Ch. 7 - Prob. 15RQCh. 7 - Prob. 16RQCh. 7 - Describe Niels Bohrs model of the structure of the...Ch. 7 - Prob. 18RQCh. 7 - Why does the equation for the energy of an...Ch. 7 - In what way was Bohrs theory a success? How...Ch. 7 - 7.21 How does the behavior of very small particles...Ch. 7 - Describe the phenomenon called diffraction. How...Ch. 7 - What experiment could you perform to determine...Ch. 7 - 7.24 What is wave/particle duality?
Ch. 7 - Prob. 25RQCh. 7 - What is the collapsing atom paradox?Ch. 7 - How does quantum mechanics resolve the collapsing...Ch. 7 - What are the names used to refer to the theories...Ch. 7 - What is the term used to describe a particular...Ch. 7 - What are the three properties of orbitals in which...Ch. 7 - What are the allowed values of the principal...Ch. 7 - What information does each type of quantum number...Ch. 7 - How does the value of n in the Rydberg equation...Ch. 7 - Why is (a) the d subshell in the Period 4...Ch. 7 - Why does every shell contain an s subshell?Ch. 7 - How many orbitals are found in (a) an s subshell,...Ch. 7 - 7.37 If the value of for an electron in an atom...Ch. 7 - 7.38 What physical property of electrons leads us...Ch. 7 - Explain the two magnetic properties that are...Ch. 7 - What is the Pauli exclusion principle? What effect...Ch. 7 - What are the possible values of the spin quantum...Ch. 7 - Suppose an electron in an atom has the following...Ch. 7 - Prob. 43RQCh. 7 - Prob. 44RQCh. 7 - Within any given shell, how do the energies of the...Ch. 7 - Prob. 46RQCh. 7 - Give the electron configurations of the elements...Ch. 7 - 7.48 Using your own words, describe how to use the...Ch. 7 - Give the correct electron configurations of (a) Cr...Ch. 7 - What is the correct electron configuration of...Ch. 7 - How are the electron configurations of the...Ch. 7 - Define the terms valence shell and valence...Ch. 7 - Why do we use probabilities when we discuss the...Ch. 7 - Sketch the approximate shape of (a) a 1s orbital...Ch. 7 - How does the size of a given type of orbital vary...Ch. 7 - How are the p orbitals of a given p subshell...Ch. 7 - What is a nodalplane? How are the number of nodal...Ch. 7 - What is a radial node? How are the number of...Ch. 7 - 7.59 How many nodal planes does a p orbital have?...Ch. 7 - On appropriate coordinate axes, sketch the shape...Ch. 7 - What is the meaning of effective nuclear charge?...Ch. 7 - *7.62 Explain why a 3s electron in Al experiences...Ch. 7 - Explain why the atomic size varies across the...Ch. 7 - Explain why cations are smaller than their...Ch. 7 - Prob. 65RQCh. 7 - Going from left to right in the periodic table,...Ch. 7 - Prob. 67RQCh. 7 - Prob. 68RQCh. 7 - Explain why ionization energy increases from left...Ch. 7 - Prob. 70RQCh. 7 - Prob. 71RQCh. 7 - Prob. 72RQCh. 7 - Why does phosphorus have a larger first ionization...Ch. 7 - Prob. 74RQCh. 7 - 7.75 For sulfur, write an equation for the change...Ch. 7 - 7.76 Why does Cl have a more exothermic electron...Ch. 7 - Prob. 77RQCh. 7 - How is electron affinity related, to effective...Ch. 7 - 7.79 What is the frequency in hertz of blue light...Ch. 7 - Ultraviolet light with a wavelength of more than...Ch. 7 - Ozone protects the earths inhabitants from the...Ch. 7 - The meter is defined as the length of the path...Ch. 7 - In New York City, radio station WCBS broadcasts...Ch. 7 - Sodium vapor lamps are often used in residential...Ch. 7 - 7.85 Calculate the energy in joules of a photon of...Ch. 7 - Calculate the energy in joules of a photon of...Ch. 7 - In the spectrum of hydrogen, there is a line with...Ch. 7 - 7.88 In the spectrum of sodium, there is a line...Ch. 7 - Use the Rydberg equation to calculate the...Ch. 7 - 7.90 Use the Rydberg equation to calculate the...Ch. 7 - Calculate the wavelength and energy in joules of...Ch. 7 - Calculate the energy in joules and the wavelength...Ch. 7 - What is the letter code for a subshell with...Ch. 7 - 7.94 What is the letter code for a subshell with...Ch. 7 - What is the value of l for (a) an f orbital and...Ch. 7 - 7.96 What is the value of for (a) a p orbital and...Ch. 7 - What are the values of n and l for the subshells:...Ch. 7 - Give the values of n and l for the subshells: (a)...Ch. 7 - For the shell with n = 6, what are the possible...Ch. 7 - 7.100 What values of are possible for a shell with...Ch. 7 - In a particular shell, the largest value of l is...Ch. 7 - What is the value of n for a shell if the largest...Ch. 7 - What are the possible values of ml for a subshell...Ch. 7 - If the value of l for an electron in an atom is 5,...Ch. 7 - If the value of ml for an electron in an atom is...Ch. 7 - How many orbitals are there in an h subshell...Ch. 7 - 7.107 Give the complete set of quantum numbers for...Ch. 7 - 7.108 Give the complete set of quantum numbers for...Ch. 7 - *7.109 In an antimony atom, how many electrons...Ch. 7 - Prob. 110RQCh. 7 - Give the electron configurations of...Ch. 7 - 7.112 Write the electron configurations of (a) As,...Ch. 7 - 7.113 Which of the following atoms in their ground...Ch. 7 - Which of the following atoms in their ground...Ch. 7 - Prob. 115RQCh. 7 - Prob. 116RQCh. 7 - Write the abbreviated electron configurations for...Ch. 7 - Write the abbreviated electron configurations for...Ch. 7 - Draw complete orbital diagrams for (a) Mg and (b)...Ch. 7 - Draw complete orbital diagrams for (a) As and (b)...Ch. 7 - 7.121 Draw orbital diagrams for the abbreviated...Ch. 7 - Draw orbital diagrams for the abbreviated...Ch. 7 - What is the value of n for the valence shells of...Ch. 7 - What is the value of n for the valence shells of...Ch. 7 - Give the configuration of the valence shell for...Ch. 7 - Give the configuration of the valence shell for...Ch. 7 - Draw the orbital diagram for the valence shell of...Ch. 7 - Draw the orbital diagram for the valence shell of...Ch. 7 - Prob. 129RQCh. 7 - Prob. 130RQCh. 7 - 7.131 Choose the larger atom in each pair: (a) Mg...Ch. 7 - Choose the larger atom in each pair: (a) Al or Ar;...Ch. 7 - Prob. 133RQCh. 7 - Place the following in order of increasing size:...Ch. 7 - Choose the larger particle in each pair:...Ch. 7 - Choose the larger particle in each pair:...Ch. 7 - Choose the atom with the larger ionization energy...Ch. 7 - Choose the atom with the larger ionization energy...Ch. 7 - Choose the atom with the more exothermic electron...Ch. 7 - Choose the atom with the more exothermic electron...Ch. 7 - 7.141 Use the periodic table to select the element...Ch. 7 - Use the periodic table to select the element in...Ch. 7 - The human ear is sensitive to sound ranging from...Ch. 7 - *7.144 Microwaves are used to heat food in...Ch. 7 - In the spectrum of hydrogen, there is a line with...Ch. 7 - *7.146 Calculate the wavelength in nanometers of...Ch. 7 - Which of the following electronic transitions...Ch. 7 - Calculate the wavelength of an electron moving at...Ch. 7 - 7.149 What, if anything, is wrong with the...Ch. 7 - 7.150 Suppose students gave the following orbital...Ch. 7 - 7.151 How many electrons are in p orbitals in an...Ch. 7 - What are the quantum numbers of the electrons that...Ch. 7 - 7.153 The removal of an electron from the hydrogen...Ch. 7 - Use orbital diagrams to illustrate what happens...Ch. 7 - *7.155 From the data available in this chapter,...Ch. 7 - 7.156 For an oxygen atom, which requires more...Ch. 7 - Write out the orbital diagram of N in the ground...Ch. 7 - The ions He+andLi2+ have line spectra that can be...Ch. 7 - A neon sign is a gas discharge tube in which...Ch. 7 - How many grams of water could have its temperature...Ch. 7 - 7.161 It has been found that when the chemical...Ch. 7 - *7.162 Using the ionization energy for sodium,...Ch. 7 - *7.163 Using photons with a wavelength of 23.7 nm,...Ch. 7 - 7.164 Our understanding of the quantum mechanical...Ch. 7 - When a copper atom loses an electron to become a...Ch. 7 - 7.166 Paired electrons cancel each others magnetic...Ch. 7 - Prob. 167RQ
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Explain why the rows in the periodic table become progressively longer as we move down the table. For example, the first row contains two elements, the second and third rows each contain eight elements, and the fourth and fifth rows each contain 18 elements.arrow_forward7. What is wrong with the statement "The atoms of element X are isoelectronic with the atoms of element Y"?arrow_forwardElements on the left side of the periodic table are more likely to form positive ions than those on the right. Use the trend in the ionization energy of the elements to explain this observation.arrow_forward
- A ceramic plate has a shiny rim. The ceramic plate is mostly composed of silicon and oxygen atoms. The shiny rim is mostly silver. When the plate is heated in a microwave oven, sparks are observed. Compare the ionization energy values of silver to those of the silicon and oxygen atoms. Explain what is happening in the oven. Why are microwaveable containers usually non-metallic? Why are most pots and pans metallic?arrow_forwardThere are many chemical concepts to explain the behavior of electrons. Electron affinity and ionization energy are two such concepts in chemistry. 1)Determine the group of element R 2)Determine the electron configuration of element R.arrow_forwardIn the table below, I1 – I6 represent first 6 ionization energies of a certain element. All units are kJ/mol. I1 I2 I3 I4 I5 I6 738 1450 7730 10500 13600 18000 This element is in the 3rd row of the periodic table, the row starting with Na. Identify the element, and explain your reasoning, based on the data in the above table.arrow_forward
- Aluminum (Al) and silicon (Si) are in the same row (period) on the periodic table. The atomic radius of aluminum is 125 pm, while the atomic radius of silicon is 110 pm. Why is the aluminum atom larger than the silicon atom? Choose the best explanation. O Aluminum contains more electrons than silicon, so the electron cloud is larger. O The valence electrons in aluminum experience a lower effective nuclear charge than those in silicon, so they aren't pulled as strongly toward the nucleus. Valence electrons in aluminum are attracted to only 13 protons, while those in silicon are attracted to 14 protons, so the valence electrons aren't pulled as strongly toward the nucleus in aluminum. O Atomic radius decreases left-to-right on the periodic table and aluminum is farther to the left.arrow_forwardAtomic radius is usually inferred from crystallographic data on elemental solids and is a crude measure of the size of the electron cloud around the nucleus. The data below are atomic radii for the elements in the second row of the Periodic Table. Explain the trend. Li : 0.152 nm Be: 0.113 nm B: 0.088 nm C: 0.077 nm N: 0.075 nm O: 0.066 nm F: 0.058 nmarrow_forwardConsider Si, S, and P.1) Based purely on ideas of electron screening and effective nuclear charge, which of these elements do you expect to have the highest first ionization energy?2) Based on experimental data, P has the highest first ionization energy. Explain this observation in terms of electron configuration arguments.arrow_forward
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