New Semester Started Get 50% OFF Study Help! --h --m --s Claim Now

Question Answers

Textbooks

Find textbooks, questions and answers

Oops, something went wrong!

Change your search query and then try again

Result Not Found

Books FREE
Study Help
Tutors
AI Study Planner NEW
Sell Books

Search
Sign In
Register

study help
sciences
introductory chemistry atoms first

Introductory Chemistry Atoms First 5th Edition Steve Russo And Michael Silver - Solutions

How many protons, electrons, and neutrons are there in:(a) 79Br (b) 81Br– (c) 23Na+ (d) 3H+
The element nitrogen has only two naturally occurring isotopes: 14N with a mass of 14.00308 amu and an abundance of 99.635% and 15N with a mass of 15.00011 amu and an abundance of 0.3650%. Calculate the atomic mass of nitrogen.
Silver has only two naturally occurring isotopes: 107Ag with a mass of 106.90509 amu and an abundance of 51.84% and 109Ag with a mass of 108.9047 amu. Calculate the atomic mass of silver
Mendeleev arranged the elements by atomic mass and then separated them into various groups. What was his criterion for which elements were grouped together?
According to the periodic table on the inside front cover, how many main-group elements are known? How many of these are representative elements?
Scandium (Sc) is a metal that tends to lose three electrons. Copper (Cu) and zinc (Zn) are also metals that tend to lose one and two electrons, respectively. Knowing this, explain why the first group in the transition metals is numbered IIIB, whereas the last two groups in the transition series are
How many electrons are there in Zr4+? What 2+ cation has the same number of electrons as Zr4+?
How many electrons are there in Br–? What 1+ cation has the same number of electrons as Br–?
Use the periodic tables to complete this table: Name of group or classification Period Group Noble gas Halogen 1 5 VIIA (17) 3 3 Elemental Atomic symbol Ne number (amu) 26 19 8 Metal Atomic metalloid, mass 01, 92 nonmetal? Metalloid
What is the identity of element X if its 2+ cation contains ten electrons?
Magnesium has a higher first ionization energy than sodium, consistent with the periodic trend for first ionization energies. Postulate a reason why Mg has the higher first ionization energy.
Calcium reacts with fluorine to form the compound CaF2. In the reaction, each atom of one of the elements loses two electrons, and each atom of the other element gains one electron.(a) Atoms of which element gain electrons?(b) Atoms of which element lose electrons?(c) What is the charge on the
A 110.99-g sample of a compound containing only calcium and chlorine is found to contain 40.98 g of calcium.(a) How many grams of chlorine are in the compound?(b) What is the percent by mass of calcium in the compound?(c) What is the percent by mass of chlorine in the compound?
Explain the major difference between Thomson’s model of the atom and Rutherford’s model. Draw a picture of each model.
Examine the periodic table that lists the first ionization energies of the elements, and state the trend for first ionization energies when you go down any group.
How does the arrangement of elements in the modern periodic table differ from that of Mendeleev’s periodic table?
Indicate atomic number, mass number, and number of protons, neutrons, and electrons in a neutral atom of each isotope: 200 2381 Al Co Au 23 U ¹1 53 1271
Write the elemental symbols for nitrogen, silicon, phosphorus, potassium, and gold.
List three properties of metals and two properties of nonmetals. Describe the behavior of metalloids relative to the behaviors of metals and nonmetals.
Explain why Rutherford expected all alpha particles to go through the gold foil undisturbed.
(a) The elements in group IA (1) are called _________________.(b) The elements in group IIA (2) are called _________________.(c) The elements in group VIIA (17) are called _________________.(d) The elements in group VIIIA (18) are called _________________.
Use Dalton’s hook atomic models to sketch a molecule of H2S.
Write the full atomic symbol for each isotope:(a) 8 protons, 9 neutrons(b) Atomic number 50, mass number 119(c) 12 neutrons, atomic number 11(d) 28 protons, mass number 58(e) 81 neutrons, symbol Ba
Complete the following statements:(a) The nucleus contains the ____________ charged particles in the atom.(b) The particles in the nucleus are the __________ and _____________.(c) Almost all of the mass of an atom is contained in the _____________.(d) The two particles whose charges cancel to make
How do metals and nonmetals differ with regard to their tendency to gain or lose electrons? With their tendency to form cations or anions?
Use the elements lithium, potassium, and sodium to explain what is meant by chemical periodicity.
There are three isotopes of hydrogen—protium, deuterium, and tritium. Protium contains one proton and no neutrons. Deuterium contains one more neutron than protium, and tritium contains one more neutron than deuterium. For each isotope, give the atomic number, mass number, number of
Given that one measure of metallic character is the tendency to lose electrons, arrange Cs, Be, Li, Ne, Na in order of increasing metallic character.
For each pair, indicate which atom loses an electron more easily:(a) Na or K(b) Na or Al(c) Rb or Ca(d) S or Cl(e) Br or Kr
Naturally occurring copper, Cu, is composed of two isotopes. The isotope copper-63 is 69.17% of naturally occurring copper and has an atomic mass of 62.94 amu. The isotope copper-65 has an atomic mass of 64.93 amu. (a) What percent of naturally occurring copper is copper-65? (b) Calculate the
Explain why the first and second statements of Dalton’s atomic theory are not exactly true.
Explain why an alternative name for the vertical columns in the periodic table is families.
Use these data to calculate the percentage of oxygen and hydrogen in these two samples of water:(a) Is the law of conservation of matter obeyed?(b) What is the percent hydrogen in water?(c) What is the percent oxygen in water?(d) Is the law of conservation of matter obeyed?(e) What is the percent
Write the following numbers in scientific notation (to prove to yourself that it sometimes saves a lot of effort by not writing zeros). Be sure you are showing the correct number of significant figures.47,100,000,000,000, assuming the uncertainty to be ±10 million
220. h × 3 = ? (the 3 is an exact number)
Do these calculations using a scientific calculator and report your answers in scientific notation: (a) (3.33 x 104 km) + (2.22 x 105 km) (b) (2.444 x 10°J) + (2.444 × 10J) (c) (2.34 x 10² m) - (2.34 x 10¹ m) (d) (4.00 x 10 L) + (6.00 x 10¹L)
A train traveling at 45.0 miles/h has to make a trip of 100.0 miles. How many minutes will the trip take? Use unit analysis to calculate your answer, and show your work.
The density of a certain liquid is 1.15 g/mL. What mass in grams of the liquid is needed to fill a 50.00-mL container? Do this problem by the method of algebraic manipulation, beginning with the equation density = mass/volume and showing all steps.
Solve the equation 5x – 6 = 3x – 8 (find the value of x that makes this equation true).
Suppose you needed someone to repeatedly make a measurement, the value of which could determine if you live or die. Suppose also that you could choose Experimenter A or Experimenter B to do the measuring. Experimenter A has the reputation of making extremely precise but woefully inaccurate
Four people listening to a 2800-word speech counted the number of words in the speech as they were listening. They came up with these results:(a) Which person was most accurate?(b) Which person was most precise?(c) Would you judge the group’s average word count as being accurate or inaccurate?(d)
There are 3 ft in a yard. A certain piece of wood is 3 ft long. What is the fundamental difference between the value of 3 ft in these two statements?
What is the uncertainty associated with the above ruler calibrated in millimeters? Explain your answer.(a) ±1 cm (b) ±0.1 cm (c) ±0.01 cm
A measured quantity is exact if(a) It is close to the true value.(b) It is precise.(c) It is measured many times.(d) All of the above.
Suppose you are teaching someone how to multiply a measured quantity such as 12.5 in. by a conversion factor that converts it to feet. Devise a general rule to tell the student how to write the conversion factor.
Two students count the grains of uncooked rice in a small cup. Both students repeat this measurement four times, with the following results:The actual number of grains is 260. Which student is more accurate? Which is more precise? Explain your answers. Mike: 256, 263, 262, 266 Ike: 250, 242, 270,
Jack is asked to determine the number of pennies in $1.00. Jill is asked to determine the number of liters in 1 gallon. Whose answer will be an exact number, and whose will be measured? Explain why.
A measured value will have uncertainty (a) Only if it is measured incorrectly.(b) If it is not measured more than once.(c) Always.(d) If the measuring device is inexpensive.
You work for a company whose job is to take inexpensive rulers, marked in centimeters, and do all that is possible to lower the uncertainty associated with measuring the diameter of a coin. List all the things that you might do. What would this do to the expense of your measuring system?
Someone is going to measure your height three times and then take an average. This height will then be fed into an automated gun that will aim 1 in. higher than your height to shoot an apple off of it. Suppose the height measurer could only be precise or accurate, but not both. Which would you
Two students attempt to measure out a quart of water into a bucket. Jack has a halfquart container, and Jill has a 10-gallon container. Which student will probably be more accurate at putting a quart of water into the bucket? Explain.
Convert the following numbers from standard to scientific notation.(a) 123 (b) 0.000 06 (c) 0.000 060 (d) 1002.0
Suppose you needed a material that could absorb heat without having its temperature increase very much. Would you choose aluminum or water? Make sure your explanation uses the concept of specific heat (somebody consult Table 2.5). Table 2.5 Specific Heats of Some
The difference between 0.1 cm and 0.10 cm is which of the following:(a) There is no difference. They are both one tenth of a centimeter.(b) There is more uncertainty in the 0.10 cm measurement.(c) There is more uncertainty in the 0.1 cm measurement.(d) 0.1 cm has uncertainty whereas 0.10 cm does
Three people measure the distance from Main Street to Market Avenue using their best estimates. Their data are 2.5 miles, 2.5 miles, and 2.6 miles. Survey charts show the actual distance to be 1.8 miles. Characterize the collected data in terms of accuracy and precision.
What is the uncertainty associated with this ruler where the numbered divisions are in centimeters?(a) ±1 mm (b) ±0.1 mm (c) ±0.01 mmWhich choice for the diameter of the coin is correct?(a) 5 × 101 mm(b) 5.0 × 101 mm(c) 5.00 × 101 mm(d) 5.000 × 101 mm cm 3 5 6
A desk is reported to weigh 185 pounds. What is the assumed uncertainty in this weight?
The measured quantity 0.00100200 seconds has (a) 9 significant figures.(b) 8 significant figures.(c) 6 significant figures.(d) 2 significant figures.
Two people attempt to measure the length in feet of a parking lot they know to be about 100 ft long. One person uses a 6-in. ruler; the other uses a 120-ft tape measure. If both measuring devices are graduated in 1/16 in., which person is likely to make the more accurate measurement? Explain.
A volume of liquid is measured as being 16.0 gallons. What is the assumed uncertainty in this measured volume?
Stop, use pencil and paper, and prove to yourself that 1.20 × 10–7 is the same as 0.000 000 120.
The measured quantity 0.00100200 s can be written as(a) 1.002 × 103 s.(b) 1.002 × 10–3 s.(c) 1.00200 × 10–3 s.(d) 1.00200 × 103 s.
A ruler is marked in intervals of 1/8 in. To what fraction of an inch can you estimate a measurement?
The voltmeter shown here is used to measure the voltage of a battery. What is the uncertainty in the measured voltage if the digits shown represent volts?(a) ±1 V (b) ±0.1 V (c) ±0.01 V
With pencil and paper, prove to yourself that if you were given the number 6.0000 × 1011, you could (a) Come up with the standard notation 600,000,000,000(b) Explain why the uncertainty is ±10 million.
The difference between 2.3 × 10–2 m and 2.30 × 10–2 m is (a) Precision (2.30 × 10–2 m is more precise).(b) Uncertainty (2.30 × 10–2 has a small uncertainty).(c) Accuracy (2.3 × 10–2 has less uncertainty).(d) None of the answers are correct.
The sum of 1.1 cm and 0.04 cm is(a) 1.14 cm.(b) 1 cm.(c) 1.1 cm.(d) 1.2 cm.
Given a written numerical value for some measurement, how do you know what the uncertainty in that measurement is?
How many interpretations are there for the number 600?
What is the result of 222 miles/2.0 h when written with the correct number of significant figures?
Unit analysis (a) Says that units are optional when writing measured quantities.(b) Says that you should analyze the units of a measurement.(c) Is a method for solving numerical problems.(d) Is a study of the number of elements in a compound.
Is it possible for a measured quantity to have no uncertainty associated with it? Explain.
How would you express 600 in. ± 1 in.?
Suppose you want to use a 100-mL beaker to fill a 2.5-L bucket with water. How many times will you have to fill your beaker?
Density(a) Is an extensive property that depends on the amount of mass of a sample.(b) Is an intensive property that does not depend on the mass or volume of the sample.(c) Can never serve as a conversion factor because it consists of two different units.(d) Has units of grams times centimeters.
What is the uncertainty in each measured number:(a) 12.60 cm (b) 12.6 cm(c) 0.000 000 03 in. (d) 125 ft
Some metals can exist in more than one form, differing in how their atoms are arranged in the solid. Shown here are two forms of the same metal. One form is denser than the other. Which is denser and why? Form A 883 000 Form B
The following is true about energy:(a) It cannot be accurately quantified.(b) It can be measured by directing it into a known mass of water.(c) Chemical change does not depend on energy; only physical change does.(d) It has units of joules per calorie.
Indicate the number of significant figures in each measurement in Problem 2.63.Data from Problem 2-63What is the uncertainty in each measured number:(a) 12.60 cm (b) 12.6 cm(c) 0.000 000 03 in. (d) 125 ft
Convert 4.68 × 10–1 to standard notation.
Suppose you have 1.0 g of water and 1.0 g of aluminum, both at 25.0°C. You want to warm them to 26.0°C. Would you need to add the same amount of heat to each? How much heat in joules would you need in each case?
Using radioactive elements, scientists determined the age of a dinosaur skeleton to be 78.5 million years. In years, what is the uncertainty in this measurement?
Convert 47.3 × 10–2 to standard notation.
Underline any trailing zeros in these measurements:(a) 12.202 km (b) 0.01 mL (c) 205°C (d) 0.010 g
Convert 47.325 × 103 to standard notation.
For the measurements in Problem 2.66, underline all the zeros that are significant.Data from Problem 2-66Underline any trailing zeros in these measurements:12.202 km 0.01 mL 205°C 0.010 g
Write the following numbers in standard notation.0.400 × 10–6
What is the uncertainty associated with each measurement in Problem 2.66?Data from Problem 2-66Underline any trailing zeros in these measurements:12.202 km 0.01 mL 205°C 0.010 g
Write the following numbers in standard notation.2.35 × 10–3
The measurement 30 ft is ambiguous, but the measurement 30. ft is not. Explain what the ambiguity is, and how adding the decimal point eliminates the ambiguity.
Give all interpretations possible for the measurement 2200 ft.
Write the following numbers in scientific notation (to prove to yourself that it sometimes saves a lot of effort by not writing zeros). Be sure you are showing the correct number of significant figures.0.000 000 000 020
Convert the following measured values from scientific notation to standard notation. For each one, indicate the number of significant figures.(a) 5.60 × 101 kg (b) 2.5 × 10–4 m(c) 5.600 × 106 miles (d) 0.02 × 102 ft
Write the following numbers in scientific notation (to prove to yourself that it sometimes saves a lot of effort by not writing zeros). Be sure you are showing the correct number of significant figures.47,100,000,000,000, assuming the uncertainty to be ±1 million
What is the uncertainty for each measured value in Problem 2.71?Data from Problem 2-71Convert the following measured values from scientific notation to standard notation. For each one, indicate the number of significant figures.5.60 × 101 kg 2.5 × 10–4 m5.600 × 106 miles 0.02 × 102 ft
Using scientific notation, write the measurement 30 ft as having an uncertainty of:(a) ±1 ft (b) ±0.1 ft (c) ±0.01 ft
27.5 in./2.0 h = ?
Using scientific notation, write the measurement 2200 ft as having an uncertainty of ±100 ft.
22.0 miles × 2.0 miles = ?
Convert the following numbers from standard notation to scientific notation:(a) 226 (b) 226.0 (c) 0.000 000 000 50(d) 0.3 (e) 0.30(f) 900,000,574 with an uncertainty of ±1 million(g) 900,000,574 with an uncertainty of ±100

Showing 2700 - 2800 of 3073

First
17
18
19
20
21
22
23
24
25
26
27
28
29
30
31

Step by Step Answers

Services

Sitemap
Fun
Definitions
Become Tutor
Used Textbooks
Study Help Categories
Recent Questions
Expert Questions
Campus Wear
Sell Your Books

Company Info

Security
Copyrights
Privacy Policy
Terms & Conditions
SolutionInn Fee
Scholarship
Online Quiz
Give Feedback, Get Rewards

Get In Touch

About Us
Contact Us
Career
Jobs
FAQ
Student Discount
Campus Ambassador

Secure Payment

Download Our App

© 2026 SolutionInn. All Rights Reserved