Chemistry In Focus
6th Edition
ISBN: 9781305084476
Author: Tro, Nivaldo J., Neu, Don.
Publisher: Cengage Learning
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Textbook Question
Chapter 3, Problem 18E
Determine the number of protons and electrons in each of the following ions:
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Element X has two stable isotopes:
35X - 75.77%, 34.97 amu
37X - 36.97%, 36.97 amu
a. Calculate the average atomic mass of X. Report your answer to 4 significant figures.
b. Using the periodic table, identify element X.
An imaginary element Saturnium, St, consists of two isotopes having masses of 101.0 amu and 104.0 amu. A sample of Saturnium was found to contain 60.0% of the St-101. What is the atomic mass of Saturnium?
A) 102.5 amu
B) 102.2amu
C) 104.0 amu
D) 102.8 amu
E) missing information
Boron (B; Z=5) has two naturally occurring isotopes. Find the percent abundances of 10B and 11B given the atomic mass of B=10.81 amu, the isotopic mass of 10B = 10.0129 amu, and the isotopic mass of 11B = 11.0093 amu. (Hint: the sum of the fractional abundances is 1. If x = abundance of 10B, then 1-x=abundance of 11B) Atomic Wt = Isotopic Mass 10B(proportion) + Isotopic Mass 11B(proportion)
Chapter 3 Solutions
Chemistry In Focus
Ch. 3 - Determining the Number of Protons and Electrons in...Ch. 3 - Prob. 3.2YTCh. 3 - Determining Protons, Neutrons, and Electrons How...Ch. 3 - Calculating Atomic Mass Magnesium has three...Ch. 3 - The Mole Concept A diamond, which is pure carbon,...Ch. 3 - The Mole Concept II Calculate the number of atoms...Ch. 3 - Prob. 1SCCh. 3 - Prob. 2SCCh. 3 - Prob. 3SCCh. 3 - Copper is composed of two naturally occurring...
Ch. 3 - Prob. 5SCCh. 3 - Which pair of elements do you expect to be most...Ch. 3 - Which statement is true of the quantum mechanical...Ch. 3 - Why is it important to understand atoms?Ch. 3 - Prob. 2ECh. 3 - What defines an element? How many naturally...Ch. 3 - Prob. 4ECh. 3 - Prob. 5ECh. 3 - Prob. 6ECh. 3 - Prob. 7ECh. 3 - Prob. 8ECh. 3 - Prob. 9ECh. 3 - Prob. 10ECh. 3 - Explain the quantum mechanical model for the atom....Ch. 3 - Give two examples of each: a. alkali metal b....Ch. 3 - Which elements exist as diatomic molecules?Ch. 3 - Explain the difference and similarity between...Ch. 3 - Prob. 15ECh. 3 - Determine the charge of each of the following: a...Ch. 3 - Determine the number of protons and electrons in...Ch. 3 - Determine the number of protons and electrons in...Ch. 3 - Give the atomic number (Z) and the mass number (A)...Ch. 3 - Prob. 20ECh. 3 - The following isotopes have applications in...Ch. 3 - The following isotopes are important in nuclear...Ch. 3 - 14C is used in carbon dating of artifacts....Ch. 3 - 40K is used to measure the age of Earth. Determine...Ch. 3 - Prob. 25ECh. 3 - Prob. 26ECh. 3 - Give electron configurations according to the Bohr...Ch. 3 - Give electron configurations according to the Bohr...Ch. 3 - Prob. 29ECh. 3 - How many valence electrons are in each element of...Ch. 3 - Prob. 31ECh. 3 - Draw electron configurations for each of the...Ch. 3 - Which two of the following elements would you...Ch. 3 - Group the following elements into three similar...Ch. 3 - We have seen that the reactivity of an element is...Ch. 3 - What is the electron configuration of Mg2+? How...Ch. 3 - Classify each of the following elements as a...Ch. 3 - Classify each of the following as a metal, a...Ch. 3 - Calculate the atomic mass of neon (Ne), which is...Ch. 3 - An element has two naturally occurring isotopes....Ch. 3 - A fictitious element has two naturally occurring...Ch. 3 - Copper has two naturally occurring isotopes. Cu-63...Ch. 3 - How many moles of titanium are present in 124 g of...Ch. 3 - Prob. 44ECh. 3 - How many moles are there in each sample? a. 45 mg...Ch. 3 - How many moles are there in each sample? a. 55.0 g...Ch. 3 - What is the mass of each sample? a.1.8 mol S...Ch. 3 - What is the mass of each sample? a.2.75 mol Fe...Ch. 3 - Determine the number of atoms in each sample....Ch. 3 - Determine the number of atoms in each sample....Ch. 3 - How many Ag atoms are present in a piece of pure...Ch. 3 - How many platinum atoms are in a pure platinum...Ch. 3 - A pure gold necklace has a volume of 1.8cm3. How...Ch. 3 - A titanium bicycle component has a volume of...Ch. 3 - An iron sphere has a radius of 3.4 cm. How many...Ch. 3 - Calculate the number of atoms in the universe. The...Ch. 3 - The introduction to this chapter states that...Ch. 3 - Suppose the absolute value of the charge of the...Ch. 3 - When we refer to doughnuts or cookies, we often...Ch. 3 - Prob. 60ECh. 3 - Why does Avogadros number have such an odd value?...Ch. 3 - Prob. 62ECh. 3 - Prob. 63ECh. 3 - Prob. 64ECh. 3 - Here are three fictitious elements and a molecular...Ch. 3 - Prob. 66ECh. 3 - Gather any two of the following items, measure...
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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
- A simple ion with a 3+ charge (for example, A13+) results when an atom (gains/loses) electrons.arrow_forwardRadon is a radioactive gas that can cause lung cancer. It has been detected in the basement of some homes. In an atom of Rn-220, (a) how many protons are there? (b) how many neutrons are there?arrow_forwardSeveral compounds containing sulfur and fluorine are known. Three of them have the following compositions: i. 1.188 g of F for every 1.000 g of S ii. 2.375 g of F for every 1.000 g of S iii. 3.563 g of F for every 1.000 g of S How do these data illustrate the law of multiple proportions?arrow_forward
- Boron (B;Z=5) has two naturally occurring isotopes. Find the percent abundances of ¹²B and ¹¹B given the atomic mass of B=1081 amu,the isotopic mass = B= 10.0129 amu, and the isotopic mass of ¹¹B=11.0093 amu.arrow_forwardA certain element X has four isotopes. 0.5600% of Xhas a mass of 83.91343amu. 9.860% of Xhas a mass of 85.90927amu. 7.000% of Xhas a mass of 86.90890amu. 82.58% of Xhas a mass of 87.90562amu. What is the average atomic mass of element X?arrow_forward6. For element X there are 3 isotopes in nature. The atomic masses in amu and the % abundance of the isotopes are given in the table below. The average atomic mass for the element will be: ELEMENT Atomic mass Abundance (%) 20X 19.9924391 90.51 21X 20.9938453 0.27 22X 21.9913837 9.22 A) 20.91 B) 16.90 C) 19.65 D) 20.18 E) 18.99arrow_forward
- an imaginary element (x) on mars is composed of 2 isotopes 34.14% of isotope x34 with a mass of 34.0 amu and isotope x37 with a mass of 37.0 amu calculate the atomic mass in Amy of the Element round your answer to 1 decimal placearrow_forwardConsider the table. Metal Tm (K) ΔHfus (kJ/mol) Tb (K) ΔHvap (kJ/mol) LiLi 454 2.99 1615 134.7 NaNa 371 2.60 1156 89.6 KK 336 2.33 1033 77.1 RbRb 312 2.34 956 69 CsCs 302 2.10 942 66 Using the data, calculate Δ?fusΔSfus and Δ?vapΔSvap for Rb.Rb. Δ?vap=ΔSvap= JK⋅molJK⋅mol Δ?fus=ΔSfus= JK⋅molarrow_forwardGa-67, an isotope of gallium (Ga), is used medically to scan for various tumors. How many protons are there in its nucleus? How many neutrons?arrow_forward
- 40Ca2+ How many protons, neutrons and electrons in this ion?arrow_forwardGallium consists of two isotopes, gallium-69 and gallium-71. Gallium-69 has a mass of 68.926 u and a fractional abundance of 0.601. Determine the mass of the gallium-71 isotope.arrow_forwardCalculate the molecular mass of the ethanol using the mass of the electrons, protons, and neutrons. (Masses of each particle and Avagadro's number are given below.)m(electron)= 9.11 x 10^(-31) kg m(proton)= 1.67 x 10^(-27) kgm(neutron)= 1.67 x 10^(-27) kgNA= 6.022 x 10^(23)arrow_forward
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