Chapter 4 Review Worksheet Answers atomic docx PDF

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Summary

average atomic mass, atomic number, number of protons, electrons, and neutrons, and significant figures...

Description

NAME

CHAPTER

4 REVIEW

WORKSHEET CALCULATE THE AVERAGE ATOMIC MASS FOR EACH ELEMENT BELOW.

# OF ELECTRONS AND # OF NEUTRONS. IN ORDER TO RECEIVE YOUR CALCULATIONS. CIRCLE OR HIGHLIGHT ALL ANSWERS.

ISOTOPE

THEN IDENTIFY THE ELEMENT’S ATOMIC NUMBER,

CREDIT, ALL CALCULATIONS MUST BE SHOWN.

MASS (AMU)

84

83.913425 85.9092624 86.9088793 87.9056143

Sr 86 Sr 87 Sr 88 Sr Average Atomic Mass Atomic Number 38 # Protons 38

# Electrons # Neutrons

ISOTOPE

38 50

MASS (AMU)

74

Se 76 Se 77 Se 78 Se 80 Se 82 Se

73.9224766 75.9192141 76.9199146 77.9173095 79.9165218 81.9167000 Average Atomic Mass Atomic Number 34 # Protons 34

% ABUNDANCE 0.46942 8.47065 6.08362 72.59246 87.6166

0.56 9.86 7.00 82.58

87.62

% ABUNDANCE 0.65791 7.11363 5.86894 18.52094 39.67635 7.15733 78.989

0.89 9.37 7.63 23.77 49.61 8.73

78.99

# Electrons # Neutrons

# OF PROTONS,

DON’T FORGET TO MAINTAIN SIGFIGS IN

34 45

NUMERIC RESPONSE:

ANSWER

3. How many protons are present in an atom of beryllium-10?

4

4. Determine the number of electrons in an atom of iridium?

77

5. What is the mass number for an oxygen atom that has 10 neutrons in its nucleus?

18

6. How many neutrons are in an atom of 235U?

143

7. What is the total number of subatomic particles in the nucleus of an atom of lead-209?

209

8. How many elements are presently recognized as of today?

118

9. COMPLETE THE FOLLOWING TABLE. ELEMENT NAME

ATOMIC NUMBER 102

PROTONS 102

ELECTRONS 102

NEUTRONS 159

METAL NONMETAL METALLOID Metal

Nobelium

No

MASS NUMBER 259

Rutherfordium

Rf

267

104

104

104

163

Metal

Y

89

39

39

39

50

Metal

Yttrium

SYMBOL

#

OF

a. b.

10. atom electron

11. a. b. c. d.

Electrons are negatively charged and are the heaviest subatomic particle. Protons are positively charged and the lightest subatomic particle. Neutrons have no charge and are the lightest subatomic particle. The mass of a neutron nearly equals the mass of a proton.

#

OF

#

OF

The smallest particle of an element that retains the properties of that element is a(n) ____. c. proton d. neutron

Which of the following is true about subatomic particles?

12. a. b. c. d.

a. b. c. d. a. b. a. b. a. b. a. b. a. b. c. d. a. b. c. d. a. b. c. d. a. b. a. b. c. d. a. b. c. d. a. b. c. d.

All atoms are ____. positively charged, with the number of protons exceeding the number of electrons negatively charged, with the number of electrons exceeding the number of protons neutral, with the number of protons equaling the number of electrons neutral, with the number of protons equaling the number of electrons, which is equal to the number of neutrons 13. The nucleus of an atom is ____. the central core and is composed of protons and neutrons positively charged and has more protons than neutrons negatively charged and has a high density negatively charged and has a low density 14. The atomic number of an element is the total number of which particles neutrons c. electrons protons d. protons and electrons 15. The sum of the protons and neutrons in an atom equals the ____. atomic number c. atomic mass nucleus number d. mass number 16. All atoms of the same element have the same ____. number of neutrons c. mass numbers number of protons d. mass 17. Isotopes of the same element have different ____. numbers of neutrons c. numbers of electrons numbers of protons d. atomic numbers 18. Which of the following statements is NOT true? Atoms of the same element can have different masses. Atoms of isotopes of an element have different numbers of protons. The nucleus of an atom has a positive charge. Atoms are mostly empty space. 19. How is the number of neutrons in the nucleus of an atom calculated? Add the number of electrons and protons together. Subtract the number of electrons from the number of protons. Subtract the number of protons from the mass number. Add the mass number to the number of electrons. 20. How do the isotopes hydrogen-1 and hydrogen-2 differ? Hydrogen-2 has one more electron than hydrogen-1. Hydrogen-2 has one neutron; hydrogen-1 has none. Hydrogen-2 has two protons; hydrogen-1 has one. Hydrogen-2 has one proton; hydrogen-1 has none. 21. What unit is used to measure weighted average atomic mass? amu c. angstrom gram d. nanogram 22. Which of the following equals one atomic mass unit? the mass of one electron the mass of one helium-4 atom the mass of one carbon-12 atom one-twelfth the mass of one carbon-12 atom 23. Which of the following statements is NOT true? Protons have a positive charge. Electrons are negatively charged and have a mass of 1 amu. The nucleus of an atom is positively charged. Neutrons are located in the nucleus of an atom. 24. The atomic mass of an element is the ____. total number of subatomic particles in its nucleus weighted average of the masses of the isotopes of the element total mass of the isotopes of the element average of the mass number and the atomic number for the element

in the nucleus?...