Basic Chemistry
6th Edition
ISBN: 9780134878119
Author: Timberlake, Karen C. , William
Publisher: Pearson,
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Question
Chapter 16, Problem 57APP
Interpretation Introduction
Interpretation:
The number of protons and neutrons in the given species needs to be determined.
Concept introduction:
- The
atomic number is the number of protons in the nucleus of the atom. - A specific element has a specific atomic number.
- The mass number is the sum of protons and neutrons in an atom.
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4.82 For each of the following, write the symbol and name for X and the number
of protons and neutrons. Which are isotopes of each other? (4.4, 4.5)
a. 124x
A
47
b. 16x
116x
49
C.
50
d. 124x
50
116X
e.
48
11:11 ÔN A D
Instructions - Classes - C...
https://coetbschemfabon.neolm.
Fill in the blanks:
(4.1) Write the complete atomic/nuclide
symbol for (a) an ion fluoride that
contains 9 protons and 10 neutrons in
the nucleus and 10 extranuclear
electrons? (b) an ion of iron that
contains 26 protons and 30 neutrons
in the nucleus and 24 extranuclear
electrons?
Note: Use the "^" caret symbol to denote
exponential components..for
Ca¯“can be written as
example, 20
"20^40Ca^-2" (atomic number written
first).
Answer: (a) mass number
nuclide symbol
(b) mass number
nuclide symbol
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Status
Dause
5.62 Write the balanced nuclear equation for
each of the following: (5.1, 5.2)
a. potassium-40 (6 decay
b. sulfur-35 (8 decay)
c. platinum-190 (a decay)
d. Ra-210 (a decay)
e. In-113m (y emission)
Chapter 16 Solutions
Basic Chemistry
Ch. 16.1 - Prob. 1PPCh. 16.1 - Prob. 2PPCh. 16.1 - Naturally occurring potassium consists of three...Ch. 16.1 - Prob. 4PPCh. 16.1 - Prob. 5PPCh. 16.1 - Prob. 6PPCh. 16.1 - Prob. 7PPCh. 16.1 - Prob. 8PPCh. 16.1 - Supply the missing information in the following...Ch. 16.1 - Prob. 10PP
Ch. 16.1 - Prob. 11PPCh. 16.1 - Prob. 12PPCh. 16.2 - Prob. 13PPCh. 16.2 - Prob. 14PPCh. 16.2 - Prob. 15PPCh. 16.2 - Prob. 16PPCh. 16.2 - Prob. 17PPCh. 16.2 - Prob. 18PPCh. 16.2 - Prob. 19PPCh. 16.2 - Prob. 20PPCh. 16.2 - Prob. 21PPCh. 16.2 - Prob. 22PPCh. 16.3 - Prob. 23PPCh. 16.3 - Prob. 24PPCh. 16.3 - Prob. 25PPCh. 16.3 - Prob. 26PPCh. 16.3 - Prob. 27PPCh. 16.3 - Prob. 28PPCh. 16.4 - Prob. 29PPCh. 16.4 - Prob. 30PPCh. 16.4 - Prob. 31PPCh. 16.4 - Prob. 32PPCh. 16.4 - Prob. 33PPCh. 16.4 - Prob. 34PPCh. 16.5 - Prob. 35PPCh. 16.5 - Prob. 36PPCh. 16.5 - Prob. 37PPCh. 16.5 - Prob. 38PPCh. 16.5 - Prob. 39PPCh. 16.5 - Prob. 40PPCh. 16.6 - Prob. 41PPCh. 16.6 - Prob. 42PPCh. 16.6 - Prob. 43PPCh. 16.6 - Prob. 44PPCh. 16.6 - Prob. 45PPCh. 16.6 - Prob. 46PPCh. 16.6 - Prob. 47PPCh. 16.6 - Prob. 48PPCh. 16.6 - Prob. 49PPCh. 16.6 - Prob. 50PPCh. 16 - Prob. 51UTCCh. 16 - Prob. 52UTCCh. 16 - The chapter sections to review are shown in...Ch. 16 - Prob. 54UTCCh. 16 - Prob. 55UTCCh. 16 - Prob. 56UTCCh. 16 - Prob. 57APPCh. 16 - Prob. 58APPCh. 16 - Prob. 59APPCh. 16 - Prob. 60APPCh. 16 - Prob. 61APPCh. 16 - Prob. 62APPCh. 16 - Prob. 63APPCh. 16 - Prob. 64APPCh. 16 - Prob. 65APPCh. 16 - Prob. 66APPCh. 16 - Prob. 67APPCh. 16 - Prob. 68APPCh. 16 - Prob. 69APPCh. 16 - Prob. 70APPCh. 16 - Prob. 71APPCh. 16 - Prob. 72APPCh. 16 - Prob. 73APPCh. 16 - Prob. 74APPCh. 16 - Prob. 75APPCh. 16 - Prob. 76APPCh. 16 - Prob. 77APPCh. 16 - Prob. 78APPCh. 16 - Prob. 79CPCh. 16 - Prob. 80CPCh. 16 - Prob. 81CPCh. 16 - Prob. 82CPCh. 16 - Prob. 83CPCh. 16 - Prob. 84CPCh. 16 - Prob. 85CPCh. 16 - Prob. 86CPCh. 16 - Prob. 87CPCh. 16 - Prob. 88CPCh. 16 - Prob. 89CPCh. 16 - Prob. 90CPCh. 16 - Consider the reaction of sodium oxalate (Na2C2O4)...Ch. 16 - Prob. 34CICh. 16 - Prob. 35CICh. 16 - Prob. 36CICh. 16 - Prob. 37CICh. 16 - Prob. 38CICh. 16 - Prob. 39CICh. 16 - Prob. 40CI
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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
- The most prevalent isotope of gold is Au-197. (4.5)a. How many protons, neutrons, and electrons are in this isotope?b. What is the atomic symbol of another isotope of gold with 116 neutrons?c. What is the atomic symbol of an atom with an atomic number of 78 and 116 neutrons?arrow_forwardThe table below is a summary of different modes of nuclear decay. Fill in the changes in atomic number (Z), number of neutrons (N), and mass number (A) in each case. Use “+” sign for increase, “–“ sign for decrease, and “0” for no change. Provide the symbol for each elementary particle involved in the decay process. (12 points) Decay Mode Particle Symbol Change in: Change in: Change in: Z N A Alpha decay 4/2α Beta decay 0/-1 β Positron decay 0/+1 β Electron capture 0/-1 earrow_forwardPart 2: Balancing Nuclear Reactions (5.2) 238 92U. 23Th + He 90 1. Identify the reactants and products in the above reaction. 2. For each element, what do the top (superscripted) and the bottom (subscripted) numbers represent respectively? 3. How many protons and neutrons are found in the uranium isotope used above? 4. How many protons and neutrons are found in the thorium isotope used above? 5. What is the difference in, a. the number of protons between U and Th? b. the number of neutrons between U and Th? c. the mass number between U and Th? 6. How do you explain these differences with respect to the nuclear reaction above?arrow_forward
- 5.64 Complete each of the following nuclear equations: (5.2) a. ? + Co Mn + He 25 27 b. ? N+ e c. e + Kr ? 241 d. He + Am →? + 2,n 2narrow_forward4.94 Indicate if each of the following statements is true or false: (4.3) a. The neutron has no net charges. b. Most of the mass of an atom is due to the protons and electrons. c. The total charge of the electrons is equal, but opposite, to the charge of the nucleus. d. The proton and the electron have about the same mass. e. The mass number is the number of protons. 4.10arrow_forwardConsider three elements with the following abbreviatedelectron configurations: (5.4, 5.5, 5.6)X = [Ar]4s23d5 Y = [Ar]4s23d104p1 Z = [Ar]4s23d104p6a. Identify each element as a metal, nonmetal, or metalloid.b. Which element has the smallest atomic size?c. Which element has the highest ionization energy?d. Which element has a half-filled sublevel?arrow_forward
- Name the element that corresponds to each of the following:(5.4, 5.5, 5.6)a. 1s22s22p63s23p64s13d5b. [Xe]6s24f 145d106p5c. halogen with the highest ionization energy d. Group 2A (2) element with the lowest ionization energye. Period 4 element with the smallest atomic sizearrow_forward5.96 a. Si b. Se c. Mn d. Sb Write the abbreviated electron configuration and group number for each of the following elements: (5.4) a. Br b. Rh c. Tc d. Raarrow_forwardPart 1: Writing Radioactive Decay Reactions (5.2) lodine-131 (131I) isotope undergoes beta decay. 1. Write the symbol for the beta particle released by iodine-131 (show the respective superscript and subscript values). 2. In the nuclear equation for beta decay of iodine-131, does the beta particle appear on the reactant or product side of the arrow? Why?arrow_forward
- 4. If you were given an antique piece of jewelry and you were told that it was made of solid gold, how could you devise a test to indicate that it was actually made of gold? 6,7.5arrow_forwardDiscussion 6 - week 6 Electron Configuration, Periodic Trends (4.7, 4.8), and Nuclear Chemistry (5.1) Part 1: Electron Configurations and Orbital Diagrams of Atoms (4.7, 4.8) 1. Write the abbreviated (short-hand) electron configuration and draw the orbital diagrams for the following ground-state (lowest energy) neutral atoms: A. Sodium (Na) B. Sulfur (S) C. Krypton (Kr) D. Vanadium (V)arrow_forward4.121 Complete the following table: (4.3) Namere is ONE O tong of the Element bots he Magnesium Joghe amouse. The Atomic Symbolbo 80 Se 228 F 88 Ra Number of Protons 28 Number of Neutrons 34 14 Number of Electrons Avearrow_forward
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