Name Period. CRHS Academic Chemistry Unit 3 - Atomic Structure & Nuclear Chemistry. Homework. Due Date Assignment On-Time (100) Late (70)

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1 Name Period CRHS Academic Chemistry Unit 3 - Atomic Structure & Nuclear Chemistry Homework Due Date Assignment On-Time (100) Late (70) Warm-Ups EC Notes, Homework, Exam Reviews and Their KEYS located on CRHS Academic Chemistry Website:

2 Page 2 of 16 WARM-UPS Unit 3 Homework #1 #6 #2 #7 #3 #8 #4 #9 #5 #10

3 Unit 3 Homework Page 3 of 16 HW 3.1 ATOMIC STRUCTURE 1. According to Dalton, what was the atom? 2. What are 2 ways that the atomic theory that is accepted today different from Dalton s Atomic Theory? 3. According to Thomson, how was the atom constructed? 4. Describe Rutherford s atomic model 5. Circle the letter of EACH sentence that is TRUE about the nuclear theory of atoms suggested by Rutherford s gold-foil experimental results. a. an atom is composed of mostly empty space b. all the positive charge of an atom is concentrated in a small central region called the nucleus c. the nucleus is composed of electrons d. the nucleus takes up a very large part of the atom e. nearly all the mass of an atom is in the nucleus 6. Describe Neils Bohr s model of the atom 7. In large part, the Bohr model described the movement and behavior of which subatomic particle? 8. The quantum model uses equations to describe the probability of finding an electron in a space around the nucleus. 9. In your own words, what was each scientist s contribution to the current atomic model science accepts today? a. Dalton b. Thomson c. Rutherford d. Bohr

4 Page 4 of 16 Unit 3 Homework 10. Label each atomic model. 1. Describe the structure of an atom. You MUST use all of the words in the box. Proton Nucleus Electron Positive Neutron Negative Electron cloud Neutral 2. What number distinguishes one element from another? 3. Define atomic number - 4. Define mass number -

5 Unit 3 Homework Page 5 of Complete the following table. Properties of Subatomic Particles Particle Symbol Charge Actual Mass (amu) proton electron neutron 6. Given the following symbol, label the mass number, atomic number, and symbol: 19 F 9 7. Rewrite the element shown in Question #6 in the form name of element mass number. 8. In a neutral atom, the number of = the number of. 9. Will changing the number of neutrons in an atom change the charge of an atom? (YES/NO). Explain. 10. Complete the chart of elements. Symb. Name Atomic # Mass # # P + # E # N 0 Shorthand Cu 64 Tin 120 U

6 Page 6 of 16 Unit 3 Homework HW 3.2 ISOTOPES AND AVERAGE ATOMIC MASS 1. Define average atomic mass - 2. Neon-20 and neon-22 are called. Specifically, how do these two atoms differ? 3. True/False In nature, all elements occur as a mixture of two or more isotopes. Isotopes of an element do NOT have a specific natural percent abundance. The average atomic mass of an element is usually closest to the atomic mass of the isotope that is most abundant. 4. Complete the chart of isotopes. Name Shorthand Atomic # Mass # # P + # E # N 0 Uranium Europium Calculate the average atomic mass of Hydrogen: % Hydrogen % Hydrogen 2 6. Calculate the average atomic mass of magnesium. Isotope Mass (u) Abundance (%) 24 Mg Mg Mg

7 Unit 3 Homework Page 7 of Chlorine, which has an atomic mass of amu, has two naturally occurring isotopes, 35 Cl and 37 Cl. Which isotope occurs in greater abundance? Explain. 8. Silver has 2 isotopes: Ag-107 with a mass of amu (52%) and Ag-109 has a mass of amu (48%). What is the average atomic mass of silver? 9. Calculate chromium s average atomic mass. Isotope Mass (amu) Abundance (%) Cr Cr Cr Cr

8 Page 8 of 16 Unit 3 Homework 3.3 ISOTOPE STABILITY AND NUCLEAR DECAY 1. An isotope that has an unstable nucleus is called a(n) 2. Use the word bank to complete the flowchart below, which describes the radioactive decay process. Word Bank Different Rays/Particles Unstable Neutrons Stable Nucleus Transmutated Energy Having too many or too few causes the of an isotope to become. The unstable nucleus undergoes a reaction and sheds by emitting. The isotope is into a more isotope of a element. 3. In your own words, what determines if a nucleus is considered stable? a. Which p + :n 0 ratio is the most stable? b. Which set of atomic # s is the most stable?

9 4. Complete the below table. Element Symbol Unit 3 Homework Page 9 of 16 Atomic # Mass # # of Neutrons Radioactive (Y/N) Th Am P Label the following elements as stable(s), marginally stable (M), or unstable(u). a. Silver b. Radon c. Cerium d. Californium e. Fluorine f. Nobelium g. Zirconium h. Uranium i. Cadmium 6. Complete the following table showing some characteristics of the types of radioactive decay. Type Consists of 2 protons and 2 neutrons High energy electron high-energy electromagnetic radiation Mass (amu) Penetrating power (low, moderate, or high) Minimum shielding

10 Page 10 of 16 Unit 3 Homework 7. Below is the alpha decay of uranium-238. a. What is the change in atomic number after the alpha decay? b. What is the change in mass number after the alpha decay? 8. Below is the beta decay of carbon-14. a. What is the change in atomic number after beta decay? b. What is the change in mass number after beta decay? 9. (T/F) Gamma radiation can penetrate the human body easily. 10 (T/F) Gamma rays have no mass and no electrical charge. 11. Look at the diagram below. Below each material indicate with a checkmark which type of radiation alpha, beta, or gamma can be stopped by each material. Paper Wood Concrete Alpha Beta Gamma

11 Unit 3 Homework Page 11 of 16 Write the equation. 1. the decay of radium-226 by alpha emission 2. the decay of plutonium-240 by alpha emission 3. the decay of carbon-14 by beta emission 4. the decay of americium-243 by alpha emission 5. the decay of uranium-235 by alpha emission 6. the decay of chlorine-32 by beta emission 7. the decay of Mg-27 by beta emission 8. the decay of chromium-49 by beta emission

12 Page 12 of 16 Unit 3 Homework 3.4 NUCLEAR REACTIONS For each characteristic, write in the blank if it describes FUSION (FU), FISSION (FI), RADIOACTIVE DECAY (RD), or NUCLEAR DISINTEGRATION (ND). 1. Very heavy nucleus is split into two approximately equal fragments 2. A decaying Polonium atom emits an alpha particle 3. Does not occur under normal conditions, + repels + 4. If not controlled nuclear explosions will occur 5. Gamma radiation emitted during beta emission 6. Advantages - inexpensive, no radioactive waste 7. 1 st controlled nuclear reaction 1942 (Chicago Pile-1 created by Enrico Fermi) 8. A decaying Uranium atom ejects high energy neutrons (n 0 ) 9. A chain reaction releases many neutrons which split more nuclei 10. If controlled, energy is released slowly 11. Neutron moderation and absorption are used to control energy flow 12. Two light nuclei combine to form single heavier nucleus 13. High energy protons (p + ) are emitted during fission of plutonium. 14. Disadvantages - requires large amounts of energy to start the reaction 15. Nuclear reactors of the future will use this form of nuclear reaction 16. Stars exhibit this kind of nuclear reaction, primarily.

13 Unit 3 Homework Page 13 of 16

14 Page 14 of 16 Unit 3 Homework

15 Unit 3 Homework Page 15 of 16 Unit 3 Extra Credit Q I T H R R C Z I S O T O P E S Z U O Z B Z Z L R G E D N F T S P R I G K M F O Y K L M O E J B Y F Z U F X X M A A B U W Z X U T V O T M I C W N D Y V F G R K X E G I V H L L L U C H F X E B P Y N H K C A H L A P U L E N U R R O N F O E N Z P B T Q W O X B T M C A O J H T M O F P K E I I W B E A J G G I R M O M R F H D U O L C N O R T C E L E M R I T D P Q Z L Q O B T R L T A L X D P O C U R N S B L A R T U E N T W O X I A E T U M E N B V E Q Q U B O K C E E Y L M N A V U G M N S A K M M Z B D I N E D W G E C T H M O T A R I U M T U K N T X C N L B R H L L U T C X N P T L E C E Y Q E Y O O M Z T Q M U H S S O D I U M S U O H R N T S M A A E T S U J O S U R S R V P O J U N S N N L X A E A I T P Z N X A E N O L S N L E P Z M D V V P Y Y A H A Q S H A V S Q D T C G F E B G T Z H V Q B J Z F The abbreviation for atomic mass unit An atom of this element has 33 protons The most basic unit of matter Equals the number of protons in an atom; identifies the element The weighted average of all isotopes of an element The average atomic mass of this element is amu An atom of this element has 4 more protons than an atom of calcium does A negatively charged subatomic particle Where electrons can be found in an atom Atoms of the same element that have different numbers of neutrons A neutral atom of this element would have 3 electrons Also known as Z, the number of protons + the number of neutrons The charge of a neutron A subatomic particle in the nucleus that has no charge Located in the center of the atom A positively charged subatomic particle The number of electrons in a neutrally charged atom of nitrogen An atom of this element has 1 less proton than an atom of magnesium The number of protons in one atom of neon The number of neutrons in an atom of potassium 39

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