1. Intro to General Chemistry

Significant Figures

Sig Fig rules (Significant Figures)

How many significant figures are in each of the following measurements?
(f) 3.8200 * 103 L

What is the number of significant figures in each of the following 
measured quantities? (d) 2.94 * 103 m2

Judge the following statements as true or false. If you believe
a statement to be false, provide a corrected version.
(g) The number 0.0033 has more significant figures than 0.033.

Round off the following quantities to the number of signifi-cant figures indicated in parentheses.
(a) 7.0001 kg (4)

Round off the following quantities to the number of signifi-cant figures indicated in parentheses.
(a) 35,670.06 m (4, 6)

Significant Figures Example 1

Which numbers are exact (and therefore have an unlimited
number of significant figures)?
a. p = 3.14
b. 12 in = 1 ft
c. EPA gas mileage rating of 26 miles per gallon
d. 1 gross = 144

How many significant figures are in each of the following measurements?
(e) 67,000 m2

How many significant figures are in each of the following measurements?
(a) 35.0445 g

How many significant figures are in each of the following measurements? (d) 510 J

Sig Fig Rules! (Significant Figures Rules and Examples)

(a) The diameter of Earth at the equator is 12756.27 km.
Round this number to three significant figures and express it
in standard exponential notation.

How many significant figures are in each of the following measurements? (b) 2000.003 g

The three targets from a rifle range shown below were produced
by: (A) the instructor firing a newly acquired target
rifle; (B) the instructor firing his personal target rifle; and
(C) a student who has fired his target rifle only a few times.
(b) For the A and C results in the future to
look like those in B, what needs to happen?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/a9736654c1f77160-1664539046628.jpg" alt="" />

For each number, underline the zeroes that are significant and
draw an x through the zeroes that are not.
a. 1,050,501 km b. 0.0020 m
c. 0.000000000000002 s d. 0.001090 cm

How many significant figures are in each number? 
a. 0.1111 s b. 0.007 m c. 108,700 km 
d. 1.563300 * 1011 m e. 30,800

Round off the following quantities to the number of signifi-cant figures indicated in parentheses.
(c) 4.995 * 103 cm (3)

There are 4 significant figures allowed in the answer to the multiplication and 3 in the subtraction.  The division is then limited by the least number of significant figures.

Correct application of the rules for significant figures in both the subtraction as well as the multiplication and division involved.

 Review the rules for significant figures in the answer to addition/subtraction problems and the rules for multiplication/division problems. 

How many significant figures should be reported for the following calculation: 5.2110 &#215; 12.20 &#247; (11.44 &minus; 2.113)

What is the number of significant figures in each of the following 
measured quantities? (b) 3 * 10-6 m

The Vehicle Assembly Building at the John F. Kennedy Space Center in Cape Canaveral, Florida, is the largest building in the world, with a volume of 3,666,500 m3
(a) Round off this quantity to four significant figures and then to two significant figures.

How many significant figures are in each of the following measurements?
(c) 0.030 03 kg

How many significant figures are in each of the following measurements? (f) 10 students

Indicate the number of significant figures in the following:&nbsp;A liter is equivalent to 1.059 qt.&nbsp;

How many significant figures are in each of the following measurements? (c) 5 ft 3 in.

Significant Figures Step by Step | How to Pass Chemistry

How to Round Numbers to Significant Figures #20

Measurement and Significant Figures

Which of the following statements uses exact numbers? (a) 1 ft = 12 in. 
(b) 1 cal = 4.184 J 
(c) The height of Mt. Everest is 29,035 ft. 
(d) The world record for the 1-mile run, set by Morocco’s Hicham el Guerrouj in July 1999, is 3 minutes, 43.13 seconds

Round off the following quantities to the number of signifi-cant figures indicated in parentheses.
(b) 68.507 g (2, 3)

The diameter of the Earth at the equator is 7926.381 mi.
(a) Round off this quantity to four significant figures and then to two significant figures.

Indicate which of the following are exact numbers: (a) the 
mass of a 3- by 5-in. index card, (b) the number of ounces 
in a pound, (c) the volume of a cup of Seattle’s Best coffee, 
(d) the number of inches in a mile, (e) the number of microseconds 
in a week, (f) the number of pages in this book.

Indicate the number of significant figures in each of the following 
measured quantities: (e) 89.2 metr ic tons

Round each number to three significant figures.
a. 79,845.82 b. 1.548937 * 107
c. 2.3499999995 d. 0.000045389

There are only two significant figures in this number.  There is another number with more than 2 significant figures.

There are only three significant figures in this number.  There is another number with more than 3 significant figures.

There are only four significant figures in this number.  There is another number with more than 4 significant figures.

Correct, this number contains five significant figures.

 Review the rules for determining significant figure, especially leading and trailing zeroes. 

Which of the following has the largest number of significant figures?

A scientist uses an uncalibrated pH meter and measures the pH of a rainwater sample four times. A different pH meter was calibrated using several solutions with known pH. The true pH of the rain was found by the calibrated pH meter to be 5.12. What can be said about the level of accuracy and precision of the uncalibrated pH meter? (LO 1.14)
<TABLE>
(a) The uncalibrated pH meter is accurate and precise. 
(b) The uncalibrated pH meter is neither accurate nor precise. 
(c) The uncalibrated pH meter is accurate but not precise. 
(d) The uncalibrated pH meter is precise but not accurate.

Assume that you have two graduated cylinders, one with a capacity of 5 mL (a) and the other with a capacity of 50 mL (b). Draw a line in each, showing how much liquid you would add if you needed to measure 2.64 mL of water. Which cylinder will give the more accurate measurement? Explain.
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/f8e08bba247156a1-1667828632065.jpg" alt="" />

How many significant figures are in each of the following measurements?
(d) 0.004 50 m

Why are Significant Figures Important?

How many significant figures are in each of the following measurements? (e) 5.10 * 102 J

How many sig figs does each number contain?a) 100. min&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;b) 17.3 x 103 mLc) 10 apples

Indicate which of the following are exact numbers: (a) the mass 
of a 32-oz can of coffee, (b) the number of students in your chemistry 
class, (c) the temperature of the surface of the Sun, (d) the 
mass of a postage stamp, (e) the number of milliliters in a cubic 
meter of water, (f) the average height of NBA basketball players.

How many significant figures are in each of the following measurements?
(b) 59.0001 cm

What is the number of significant figures in each of the following 
measured quantities? (e) 92.03 km

Round each of the following numbers to three significant 
figures and express the result in standard exponential notation: 
(e) -0.00000324683.

Round off the following quantities to the number of signifi-cant figures indicated in parentheses.
(d) 2,300,000.1 (7)

Round each of the following numbers to three significant
figures and express the result in standard exponential notation:
(a) 2048732.23

Two students determine the percentage of lead in a sample
as a laboratory exercise. The true percentage is 22.52%. The
students’ results for three determinations are as follows:
(1) 22.52, 22.48, 22.54
(2) 22.64, 22.58, 22.62
(b) Precision can be judged by examining the average of the
deviations from the average value for that data set. (Calculate
the average value for each data set; then calculate the average
value of the absolute deviations of each measurement
from the average.) Which set is more precise?

Which numbers are exact (and therefore have an unlimited 
number of significant figures)? 
a. p = 3.14 
b. 12 in = 1 ft 
c. EPA gas mileage rating of 26 miles per gallon 
d. 1 gross = 144

How many significant figures are in each of the following measurements? (a) $130.95

Is the use of significant figures in each of the following statements
appropriate? (a) The 2005 circulation of National Geographic
was 7,812,564.

How many significant figures are contained in the following measurement?&nbsp;3,482,005 mg&nbsp;

Significant Figures and Zero (1.3)

Round off the following quantities to the number of signifi-cant figures indicated in parentheses.
(d) 2.309 85 * 10-4 kg (5)

Round off the following quantities to the number of signifi-cant figures indicated in parentheses.
(b) 1.605 km

Round off the following quantities to the number of signifi-cant figures indicated in parentheses.
(c) 13.2151 g/cm3 (3)

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2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

SI Units

The International System of Units (SI) is related to the metric system and is based on seven base units.

Physical & Chemical Changes

A physical change involves a change in the phases of matter, whereas a chemical change involves a change in chemical bonds.&nbsp;

Physical Properties

Physical Properties are measurable properties that describe the state of chemical compounds.&nbsp;

Significant Figures: In Calculations

Significant Figures are often involved in chemical calculations.&nbsp;

Scientific Notation

Scientific Notation is used to turn small or large inconvenient numbers into manageable ones.&nbsp;

Density of Non-Geometric Objects

The density of non-geometric objects can be determined using water displacement.&nbsp;

Density

Density represents the mass of an object or compound within a given volume.&nbsp;

Significant Figures: Precision in Measurements

Significant Figures are used to discuss the level of precision in any measurement.&nbsp;

Intensive vs. Extensive Properties

Intensive Properties are independent and Extensive Properties are dependent on the size or amount of substance present

Density of Geometric Objects

The density of geometric objects generally includes spheres, cubes and cylinders.&nbsp;

Significant Figures are used to determine some level of accuracy within our recorded measurements.&nbsp;

Dimensional Analysis

We use dimensional analysis&nbsp;as a fail proof process to convert from one unit to another.

Chemical Properties

Chemical Properties are observed during chemical reactions.&nbsp;

Temperature

Temperature is a measure of the amount of average kinetic energy of the atoms in a compound.

Metric Prefixes

Metric Prefixes are “labels” that can be placed in front of base units.&nbsp;

Conversion Factors

Conversion Factors represent ratios or fractions composed of different units.&nbsp;

Classification of Matter

Chemistry is the study of matter and the changes it undergoes, with the atom being its basic functional unit.&nbsp;