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Home , Inorganic chemistry

CHEM 110 Week 1 Inorganic I , Elements, and Compounds

Week 1 Reading Assignment

Your week 1 reading assignment has been selected from chapters 3 and 5 in your textbook. As part of your reading assignment, you are expected to work the sample problems and the selected “questions and problems” at the end of your book sections. The answers to the odd numbered “questions and problems” can be found at the end of your book chapters. You should use this key to check yourself. If you are having problems arriving at the correct answer as listed in the back of your book chapter, please email me.

 Read section 3.1 and answer the odd numbered “questions and problems” on page 85.  Read section 3.2 and answer the odd numbered “questions and problems” on page 91.  Read section 3.3 and answer “questions and problems” 3.15 and 3.17 on page 94. You do not have to know the experimental details used to determine the structure of an .  Read section 3.4 and answer the odd numbered “questions and problems” on page 97.  Read about and atomic mass in section 3.5 and answer “questions and problems” 3.29 and 3.31 on page 100. Skip the part on calculating atomic mass using isotopes.  Read section 3.6.  Read section 3.7.  Read about “ Number and Valence ” and “-Dot Symbols” in section 3.8. Answer “questions and problems” 3.57 and 3.59 on page 118.

 Read section 5.1 and answer the odd numbered “questions and problems” on page 163 and 164.  Read section 5.2 and answer the odd numbered “questions and problems” on page 166.  Read section 5.3. You will not be responsible for naming ionic formulas. Answer “questions and problems” 5.17 and 5.23 on page 170.  Read section 5.4 and answer “questions and problems” 5.31 on page 174. Skip the part about naming compounds containing polyatomic .  Read pages 175 – 178 of section 5.5 and answer “questions and problems” 5.37 and 5.39.  Skip section 5.6.  Read section 5.7 and answer “questions and problems” 5.53, 5.55, and 5.57.  Skip section 5.8 and 5.9.

Week 1 Study Guide

As stated in your syllabus, the tests in this class are closed-notes, closed-book, and closed to internet searches. In addition, you are not allowed to work together. The learning objectives provided below should be mastered before you take the week 1 quiz. For your convenience, the learning objectives for week 1 will be followed by helpful hints and/or sample test questions so that you can get a feel for what

Dr. Gryzenia the week 1 quiz in this class will be like. An electronic will be provided as needed on the quiz to help you answer some of the questions. The periodic table that will be provided is shown below:

Before taking the week 1 quiz, you should be able to meet the following learning objectives:

Chapter 3

 Memorize the names and correct spelling of the following 15 elements: calcium (Ca), (C), chlorine (Cl), fluorine (F), gold (Au), (H), iron (Fe), lead (Pb), nitrogen (N), oxygen (O), (P), potassium (K), silver (Ag), (Na), and (S). [Chapter 3.1]

 Memorize the chemical symbols of the following 15 elements: calcium (Ca), carbon (C), chlorine (Cl), fluorine (F), gold (Au), hydrogen (H), iron (Fe), lead (Pb), nitrogen (N), oxygen (O), phosphorus (P), potassium (K), silver (Ag), sodium (Na), and sulfur (S). [Chapter 3.1]

Quiz Me 1. What is the chemical symbol for potassium?

Quiz Me 2: What is the chemical symbol for silver?

 Use the periodic table to identify the groups and periods. [Chapter 3.2] Helpful hint: Periods are used as punctuation at the end of some sentences. Sentences are written in a horizontal fashion, just like the rows within the periodic table. If you associate periods with horizontal sentences, then it will help you remember that the horizontal rows in the periodic table are called periods.

Dr. Gryzenia Quiz Me 3: Give the period and group number for Au. On the test, the periodic table will be provided to help you answer this question. A. Period 1B (11), Group 6 B. Period 1B (11), Group 5 C. Period 6, Group 1B (11) D. Period 5, Group 1B (11)

 Identify elements as transition elements, alkali metals, alkaline earth metals, halogens, and noble . [Chapter 3.2]

Quiz Me 4: Which one of the following is an alkaline earth metal? On the test, the periodic table will be provided to help you answer this question. A. Chlorine B. Calcium C. Nitrogen D. Sodium E. Iron

 Describe the physical properties of alkali metals, alkaline earth metals, halogens, and noble gases. [Chapter 3.2]

Quiz Me 5: Which one of the following reacts vigorously with and forms white products when they combine with oxygen? A. the halogens B. the noble gases C. the alkali metals D. the transition elements E. the alkaline earth metals

 Define metal, nonmetal, and metalloid and classify elements as metal, nonmetal, or metalloid. [Chapter 3.2] Helpful hint: Table 3.3 in your textbook does a nice job of comparing and contrasting metals, nonmetals, and metalloids.

Quiz Me 6: Which one of the following is the best conductor of heat and electricity? A. metal B. metalloid C. nonmetal

Dr. Gryzenia Quiz Me 7: Which one of the following is the best conductor of heat and electricity? On the quiz, the periodic table will be provided to help you answer this question. A. Chlorine B. Silicon (Si) C. Calcium D. Arsenic (As) E. Fluorine

 Define atom, compound, , electron, proton, neutron, and nucleus. [Chapter 3.3]

Quiz Me 8: Which one of the following is negatively charged? A. proton B. atom C. electron D. nucleus E. neutron

 Discuss Dalton’s atomic theory and know the type of microscope that is needed to visualize an atom. [Chapter 3.3] Interesting fact: The inventors of this type of microscope won the Nobel Prize in Physics in 1986.

 Describe the structure and organization of the atom. [Chapter 3.3] Helpful Hint: Use Figure 3.10 in your textbook the help you visualize the structure and the organization of the atom.

Quiz Me 9: Which of the following is TRUE about the organization of the atom? A. Neutrons are found within the nucleus of an atom. B. Electrons are found within the nucleus of an atom. C. Protons are found within the nucleus of an atom. D. A and C are TRUE. E. B and C are TRUE.

 Define atomic mass unit (amu) and Dalton (Da), and know the relative mass of the proton, neutron, and electron. [Chapter 3.3]

Quiz Me 10: Which one of the following is TRUE? A. An amu is defined as 1/12 of the mass of the hydrogen atom. B. An amu is defined as 1/12 of the mass of the carbon atom. C. An amu is defined as 1/12 of the mass of the sulfur atom. D. An amu is defined as 1/12 of the mass of the phosphorus atom. E. An amu is defined as 1/12 of the mass of the oxygen atom.

 Explain the meaning of the atomic number. [Chapter 3.4]

Dr. Gryzenia Quiz Me 11: What is the atomic number for the element oxygen? On the quiz, the periodic table will be provided to help you answer this question. A. 76 B. 16 C. 14 D. 8 E. 2

 Explain the meaning of the mass number. [Chapter 3.4] Helpful hint: Since electrons are so small, they essentially contribute zero to the mass of an atom. The mass number of an atom is the number of protons plus the number of neutrons. Keep in mind that the mass number is always larger than the atomic number.

 Given the atomic number and the mass number of an atom, calculate the number of protons, neutrons, and electrons… and vice versa. [Chapter 3.4]

Quiz Me 12: How many protons are in a neutral bromine (Br) atom that has a mass number of 80? On the quiz, the periodic table will be provided to help you answer this question.

Quiz Me 13: How many electrons are in a neutral bromine (Br) atom that has a mass number of 80? On the quiz, the periodic table will be provided to help you answer this question.

Quiz Me 14: How many neutrons are in a neutral bromine (Br) atom that has a mass number of 80? On the quiz, the periodic table will be provided to help you answer this question.

 Define , write and recognize atomic symbols for a given isotope, and give the number of protons, neutrons, and electrons in one or more of the isotopes of an element. [Chapter 3.5]

Quiz Me 15: Give the number of neutrons in C-14. On the quiz, the periodic table will be provided to help you answer this question.

 Describe the energy levels and sublevels for the electrons in an atom. [Chapter 3.6]

Quiz Me 16: Which one of the following sublevels has the lowest energy level? A. the p sublevel B. the d sublevel C. the s sublevel D. the f sublevel

 Define valence electrons and determine the number of valence electrons in a given element. [Chapter 3.8]

Quiz Me 17: How many valence electrons are in (Mg)?

 Identify electron dot symbols for the elements. [Chapter 3.8]

Dr. Gryzenia Chapter 5

 Know when ionic and covalent bonds occur. [Chapter 5.1]

 Define , ionic charge, cation, anion, and . [Chapter 5.1] Helpful hint: the octet rule describes the tendency for elements in Groups 1A – 7A (1, 2, 13 – 17) to react with other elements to produce a stable electron configuration, usually eight electrons in the outer shell (page 198).

Quiz Me 18: Which one of the following is a negatively charged ion of a nonmetal? A. anion B. cation C. proton D. neutron E. electron

 Use the octet rule to determine how many electrons must be lost or gained to obtain a stable electron configuration. Helpful hint: The atoms of the elements in Group 1A (1) lose one electron to form ions with a 1+ charge. The atoms of the elements in Group 2A (2) lose 2 electrons to form ions with a 2+ charge. The atoms of the elements in Group 3A (13) lose 3 electrons to form ions with a 3+ charge. The atoms of the non-metals in Group 7A (17) gain one electron to form ions with a 1- charge. The atoms of the elements in Group 6A (16) gain two electrons to form ions with a 2- charge. The atoms of the elements in Group 5A (15) typically gain three electrons to form ions with a 3- charge. [5.1]

Quiz Me 19: How many electrons must be lost by atoms of the element (Li) to obtain a stable electron configuration? On the quiz, the periodic table will be provided to help you answer this question.

 Recognize ionic symbols for atoms of elements in Groups 1A (1), 2A (2), 3A (13), 5A (15), 6A (16), and 7A (17). [Chapter 5.1]

Quiz Me 20: Which one of the following represents the symbol for the ion of potassium? On the quiz, a periodic table will be provided to help you answer this question. A. K1+ B. K2+ C. K3+ D. K2- E. K1-

 Define and ionic bond. [Chapter 5.2]

 Determine the ionic charges for an atom, and use charge balance to write the correct formula for an ionic compound. [Chapter 5.2] You may find the following YouTube video helpful: https://www.youtube.com/watch?v=mHkrPT_NFCQ Another helpful hint: I like to use the cross- down method of writing ionic compounds. Let’s use the example that your book gives on page 165. In order to write an ionic compound containing sodium (Na+) and sulfur (S2-), we can cross-down the exponents as shown on the following page:

Dr. Gryzenia

We can also do the cross-down method to work the concept check 5.2 on page 166:

Dr. Gryzenia Quiz Me 21: Which one of the following represents the correct ionic formula for the compound formed between Al3+ and Cl-?

A. ClAl3

B. Cl3Al

C. AlCl3

D. Al3Cl

 Identify cations and anions in a formula. [Chapter 5.3]

 Determine the variable charge of transition elements within a formula. [Chapter 5.3] Hint: See the

CuCl2 example on page 168 of your textbook.

 Define polyatomic ion, and recognize the following as polyatomic ions: hydroxide (OH-), ammonium + - - 2- 2- 3- (NH4 ), nitrate (NO3 ), chlorate (ClO3 ), (CO3 ), (SO4 ), (PO4 ). [Chapter 5.4]

 Distinguish ions from polyatomic ions. [Chapter 5.4] Helpful hint: an ion that contains two capital letters contains two elements that are covalently bonded together; therefore it is a polyatomic ion.

Quiz Me 23: Which one of the following is a polyatomic ion? A. Na+ B. OH- - C. ClO2 D. A and C E. B and C

 Write the formula of a compound that forms between ions and polyatomic ions. [Chapter 5.4] Helpful hint: You can use the cross-down method for writing formulas for compounds containing ions and polyatomic ions. Let’s use the example that your book gives on page 172. In order to write 2+ - an compound containing Mg (ion) and NO3 (polyatomic ion), we can cross-down the exponents as shown on the following page:

Dr. Gryzenia

3- + Quiz Me 24: What is the formula for the compound containing and PO4 and Na ?

A. Na3PO4

B. Na(PO4)3

C. PO4Na3

D. (PO4)3Na

 Define covalent compound, covalent bond, , and diatomic, and give examples of elements that are most likely to form covalent compounds. [Chapter 5.5]

Quiz Me 25: Which one of the following elements is most likely to form a covalent compound? On the quiz, a periodic table will be provided to help you answer this question. A. Ag B. C C. Fe D. Au

 Know the number of valence electrons, bonding pairs, and lone pairs in an electron dot formula. [Chapter 5.5]

Quiz Me 26: How many valence electrons, bonding pairs, and lone pairs are in H:H? A. valence electrons = 1, bonding pairs = 0, lone pairs = 1 B. valence electrons = 1, bonding pairs = 1, lone pairs = 0 C. valence electrons = 2, bonding pairs = 0, lone pairs = 1 D. valence electrons = 2, bonding pairs = 1, lone pairs = 0

Dr. Gryzenia  Define electronegativity and use the periodic table to describe trends in electronegativity. [Chapter 5.7]

Quiz Me 27: Which one of the following has the highest electronegativity? On the quiz, a periodic table will be provided to help you answer this question. A. Sr B. Ba C. Be D. Mg

 Define polar and nonpolar covalent bonds. [Chapter 5.7] Helpful hint: Table 5.14 is a nice illustration of polar and nonpolar covalent bonds.

 Given the electronegativity difference, determine whether a bond is polar, nonpolar, or ionic. [Chapter 5.7]

Quiz Me 28: If the difference in electronegativity between 2 non-metals is 0 then what type of bond is formed? A. polar covalent bond B. nonpolar covalent bond C. ionic bond

Answers to the Quiz Me questions

1. K 2. Ag 3. C 4. B 5. C 6. A 7. C 8. C 9. D 10. B 11. D 12. 35 13. 35 14. 45 15. 8 16. C 17. 2 18. A 19. 1 20. A

Dr. Gryzenia 21. C 22. B 23. E 24. A 25. B 26. D 27. C 28. B

Dr. Gryzenia