Chem Unit 2 Homework Questions

Lesson 33 pages 169-173 Question 4: Create a four-carbon molecule that is... a.) an alkane (draw on paper)

c4h10 (Butane) (check book/slader)

Lesson 24 pgs. 116-121 Question 3: How is the arrangment of electrons in an atom related to the location of the atom on the periodic table?

The number of electron shells in an atom is the same as the number of the period where the element is located on the periodic table, also each section of the periodic table corresponds to a particuar subshell of electrons.

Lesson 20 pages 98-102 Question 1: How can you use valence electrons to predict which ionic compounds will form?

The number of valence electrons can predict whether an atom will form a cation or anion, as well as the size of the charge on the ion. Ionic compounds form between cations and anions in a ratio so that the charges are balanced.

Lesson 18 pages 88-92 Question 1: How can you determine the arrangement of an element's electrons from its position on the periodic table?

The period that it is in will determine the number of shells in the atom and the group number will tell you how many valence electrons the atom has, so you can figure out the total number of electrons in the atom.

Lesson 18 pages 88-92 Question 3: What do Be, Mg, and Ca all have in common?

They all are in group 2A so they all have two valence electrons and because of this, they have similar properties.

Lesson 24 pgs. 116-121 Question 1: What are electrons subshells?

They are divisions within a specific electron shell of an atom, there are specific names for each subshell, s, p, d, and f

Lesson 24 pgs. 116-121 Question 10: Explain why the chemical properties of argon, krypton, and xenon are similar, even though there are 18 elements between argon and krypton, and 32 elements between krypton and xenon.

They each have eight valence electrons

Lesson 19 pages 93-97 Question 11: What is the symbol of an ion with 22 protons, 24 neutrons, and 18 electrons?

Ti^4+

Lesson 32 pages 165-168 Question 2: What is the octet rule, and how can you use it to create a molecular structure?

When atoms bond covalently to form molecules, they share electrons to obtain an electron arrangement similar to that of a noble gas atom. This tendency to bond until eight valence electrons surround an atom is called the octet rule Creating a molecular structure using the Octet Rule : - Now, as all the central atoms have 8 electrons once the compound is formed, it is easy to determine the number of bonds that an element will make from it's valency. -Suppose the valency is 4, as in case of Carbon, then the element requires an additional 4 electrons and thus will make 4 covalent bonds. -In this way, by figuring out this information for all the elements contained in the molecule, we can construct the structure of a molecule using the Octet Rule.

Lesson 20 pages 98-102 Question 3: Lithium Nitride has the formula Li3N. a.) what is the charge on the lithium ion? b.) what is the charge on the nitrogen atom? c.) show that the charges on the ions add up to zero. d.) What is the total number of valence electrons in all the atoms in Li3N?

a.) +1 b.) -3 c.) Lithium nitride has 3 lithium ions with the charge of +1 and and 1 nitride ion with the charge -3. 3(+1) + (-3) = 3 + (-3) = 0 d.) 8 valence electrons because there are 3 lithium atoms and each one has 1 valance electron plus one nitride atom which has 5 valence electrons.

Lesson 20 pages 98-102 Question 4: Aluminum arsenide has the formula AlAs. a.) What is the charge on the aluminum ion? b.) What is the charge on the arsenic ion? c.) show that the charges on the ions add up to zero. d.) What is the total number of valence electrons in all the atoms in AlAs?

a.) +3 b.) -3 (to make the compound neutral) c.) +3 (1) + -3 (1) = 0 d.) Al has 3 valence electrons and As has 5 valence electrons so when you add them up you get 8 valence electrons total in AlAs.

Lesson 24 pgs. 116-121 Question 9: consider the element with the atomic number 13... a.) What is the electron configuration for this element? b.) How many valence electrons does it have? how do you know this? c.) How many core electrons does it have? How did you figure it out?

a.) 1s^2 2s^2 2p^6 3s^2 3p^1 b.) Element 13 has 3 valence electrons because it has three electrons in the outer shell, n=3 c.) Element 13 has 10 core electrons because it has 2 shells filled completely, n=1 with 2 electrons and n=2 with 8 electrons

Lesson 20 pages 98-102 Question 6: What are the total numbers of valence electrons in all the atoms in each of these compounds? a.) KBr b.) CaO c.) Li2O d.) CaCl2 e.) AlCl3

a.) 8 b.) 8 c.) 8 d.) 16 e.) 24

Lesson 21 pages 103-108 Question 7: Predict the formulas for the ionic compounds that are formed when these metals and nonmetal elements are combined. Name each compound. a.) Al and Br b.) Al and S c.) Al and As d.) Na and S e.) Ca and S f.) Ga and S

a.) AlBr3, aluminum bromide b.) Al2S3, Aluminum sulfide c.) AlAs, Aluminum arsenic d.) Na2S, Sodium sulfide e.) CaS, Calcium sulfide f.) Ga2S3, Gallium sulfide

Lesson 22 pages 109-111 Question 3: Write the name for each ionic compound listed here... a.) NH4Cl b.) K2SO4 c.) Al(OH)3 d.) MgCO3

a.) Ammonium Chloride b.) Potassium Sulfate c.) Aluminum Hydroxide d.) Magnesium Carbonate

Lesson 29 pgs 151-155 Question 5: Structural formulas for six molecules are shown below. Write the molecular formula for each of the molecules. (look in book)

a.) C3H6O2 b.) C5H10O c.) C4H10O d.) C4H8O2 e.) C4H11N f.) C2H4O2

Lesson 18 pages 88-92 Question 6: see hw

a.) Carbon has 6 electrons and Silicon has 14 electrons because that is their atomic number b.) (picture) c.) They both have 4 valence electrons d.) Carbon has 2 core electrons and Silicon has 10 core electrons e.) The properties of Carbon and Silicon are similar because they are in the same group and they have the same number of valence electrons.

Lesson 21 pages 103-108 Question 8: For each compound, write the cation and anion with the appropriate charge. Then write the chemical formula for each compound. a.) magnesium oxide b.) rubidium bromide c.) strontium Iodide d.) beryllium fluoride e.) aluminum chloride f.) lead sulfide

a.) Cation: Mg^2+, Anion: O^2-, MgO b.) Cation: Rb+, Anion: Br-, RbBr c.) Cation: Sr^2+, Anion: I-, SrI2 d.) Cation: Be^2+, Anion: F-, BeF2 e.) Cation: Al^3+, Anion: Cl-, AlCl3 f.) Cation: Pb^2+, Anion: S2-, PbS

Lesson 18 pages 88-92 Question 7: see hw

a.) Chlorine, Cl, Group 7A b.) 17 protons, because the atomic number is 17 c.) 18 neutrons, because the average atomic mass is 35.45 which rounds to 35 and 35-17=18 (subtracted protons from mass) d.) 17 electrons, because the atomic number is 17 e.) 7 valence electrons, because it is in group 7A f.) 10 core electrons, because 17-7=10 g.) Fluorine, Bromine, and Iodine, because they are all in the same group

Lesson 24 pgs. 116-121 Question 13: Which elements are described by these electron configurations?... a.) 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^4 b.) 1s^2 2s^2 2p^6 3s^2 3p^2 c.) 1s^2 2s^2 2p^3 d.) 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^65s^2 4d^10 5p^6 6s^1 e.) 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^2 4f^14 5d^10 6 p^2 f.) (Kr)5s^2 4d^9

a.) Chromium b.) Silicon c.) Nitrogen d.) Cesium e.) Lead f.) Silver

Lesson 19 pages 93-97 Question 16: Which of these ions have the same number of electrons as S^2-? a.) Cl- b.) Ca^2+ c.) Na+ d.) O^2- e.) P^3-

a.) Cl- b.) Ca^2+ e.) P^3- (all add up to 18 electrons)

Lesson 20 pages 98-102 Question 7: Explain why the following compounds do not form. a.) NaCl2 b.) CaCl c.) AlO

a.) It has the net charge of +1 because Na has the charge -1 and Cl has the charge -1 for each atom and there are 2 so 2(-1) + 1(+1) = -1 b.) It has a net charge of 1 because Ca has the charge +2 and Cl has the charge -1 so 1(+2) + 1(-1) = 1 c.) It has a net charge of +1 because Al has the charge +3 and O has the charge -2 so 1(+3) + 1(-2) = +1

Lesson 22 pages 109-111 Question 4: Write the chemical formula for each compound listed here... a.) lithium sulfate b.) potassium hydroxide c.) magnesium nitrate d.) ammonium sulfate

a.) Li2SO4 b.) KOH c.) Mg(NO3)2 d.) (NH4)2SO4

Lesson 32 pages 165-168 Question 7: Consider the molecules C2H2, N2H2, and H2O2. a.) Draw Lewis dot structures for each, what pattern do you notice? b.) What can you do to check that your Lewis dot structures are correct? Name at least 2 ways. (draw on paper)

a.) Pattern: All follow the octet rule b.) count and make sure the octet is fulfilled, count the dots

Lesson 19 pages 93-97 Question 15: Which of these ions have the correct charge? a.) Na^2+ b.) Li+ c.) Al^4+ d.) Ca^2+ e.) Ga^3+

b.) Li+ d.) Ca^2+ e.) Ga^3+

Lesson 18 pages 88-92: Question 10: What do the elements in period 3 have in common? a.) Their atoms have the same number of valence electrons b.) Their atoms have the same number of electron shells c.) Their atoms have the same properties d.) None of the above

b.) Their atoms have the same number of electron shells

If two chemical samples both produce an orange flame upon testing, which statement is true? a.) the two samples contain identical compounds b.) The samples both contains chlorine atoms c.) The samples both contain calcium atoms d.) The samples both contain potassium atoms e.) The samples both contain different compounds

c.) The samples both contain calcium atoms

Lesson 33 pages 169-173 Question 4: Create a four-carbon molecule that is... c.) an alcohol (draw on paper)

c4h10o Isobutanol (check book/slader)

Lesson 33 pages 169-173 Question 4: Create a four-carbon molecule that is... d.) an ester (draw on paper)

c4h8o2 Ethyl acetate (check book/slader)

Lesson 18 pages 88-92 Question 9: If an element is located in Group 4A of the periodic table, what can you conclude about the atoms of this element? a.) It has 4 valence electrons b.) It has 4 electron shells c.) It has four core electrons d.) It has properties similar to carbon e.) Both A and D

e.) Both A and D

Lesson 19 pages 93-97 Question 1: What is the difference between an anion and a cation?

-An anion is an ion with a negative charge - It is an anion when atoms gain electrons - Anions are mostly nonmetals -A cation is an ion with a positive charge. -It is a cation when atoms lose electrons - Cations are mostly metals

Lesson 28 pgs 146-150 Question 1: How do scientist classify smells? What purpose might this serve?

-by putting similar types of smells into categories -It allows scientists to talk about them in a consistent way

Lesson 21 pages 103-108 Question 5: Give examples of 3 ionic compounds with a metal to nonmetal ratio of 2:1. Specify the total number of valence electrons for each compound. Name each compound.

1.) Li2O, lithium oxide, 8 valence electrons 2.) Na2S, sodium sulfide, 8 valence electrons 3.) K2Se, potassium selenium, 8 valence electrons

Lesson 22 pages 109-111 Question 2: How can you tell from a chemical formula if there is a polyatomic ion in a compound?

A polyatomic ion will have more than one bonded together, also when it contains two or more of the same polyatomic ion, that ion is written in parentheses with the subscript written outside the parentheses

Lesson 20 pages 98-102 Question 2: How does the rule of zero charge help you predict the formula of an ionic compound?

Because you know that what anion is present, the cation that bonds with it will make the net charge zero.

Lesson 18 pages 88-92 Question 4: Draw a shell model for B. Identify the core and valence electrons.

Boron has 2 core electrons and 3 valence electrons

Lesson 24 pgs. 116-121 Question 7: What is the outermost subshell for bromine, Br?

Br's electron configuration is [Ar] 4s2 3d10 4p5. Therefore, 4p is its outer subshell.

Lesson 32 pages 165-168 Question 9: Which is more likely to exist in nature, a molecule of CH3 or a molecule of CH4? Explain your reasoning.

CH4 would form a stable compound because all of the atoms in the molecule are surrounded by the most stable number of valance electrons - eight for carbon, two for hydrogen. In CH3, the carbon atom would have only seven electrons in its outer shell.

What evidence do you have from flame tests that copper is responsible for producing a flame with a blue-green color?

Copper is the metal in all of the compounds that create a blue-green color, so copper is what is responsible for it.

Lesson 19 pages 93-97 Question 13: Explain why the element on the right side of the periodic table gain electrons instead of losing them.

Elements on the right side of the table do not tend to lose electrons because the charge would be too large because they have more core electrons than the left side elements.

Lesson 19 pages 93-97 Question 8: List 4 ions that have the same number of electrons as neon, Ne.

F-, O^2-, N^3-, Na+

Lesson 24 pgs. 116-121 Question 8: Name an element with electrons in the f subshell.

Gadolinium (Gd)

Lesson 28 pgs 146-150 Question 8: What do you think 1,5-pentanedithiol (C5H12S2) would smell like? How confident are you of your answer? Explain why.

I think it would smell bad because it has sulfur in it which I know is known for smelling bad.

Lesson 24 pgs. 116-121 Question 4: How many subshells are in each shell: n=1 n=2 n=3 n=4

If n= 1, there is one subshell and it is s subshell If n=2 , there are two subshells and they are s and p If n=3 , there are three subshells and they are s,p and d If n=4 , there are four subshells and they are s,p,d and f

Lesson 22 pages 109-111 Question 1: What is a polyatomic ion?

Ionic compounds that consist of two or more elements.

Lesson 24 pgs. 116-121 Question 5: What is the total number of subshells for elements in period 5 of the periodic table?

It will have 5 shells so there would be 15 subshells

Lesson 18 pages 88-92 Question 2: If you know what group and element is in, what can you predict about its electron arrangement?

It will have that many valence electrons on the valence shell.

Imagine that you were in charge of creating a red and purple fireworks display. Name two combinations of compounds you could use.

Lithium Nitrate and Potassium Nitrate

Lesson 28 pgs 146-150 Question 2: How are molecular formulas related to smell? How are chemical names related to smell?

Molecular Formulas: The number of atoms of each element relate, and the type of element also relates Chemical Names: The endings relate to certain smell categories

Lesson 29 pgs 151-155 Question 2: What are isomers?

Molecules with the same molecular formula and different structural formula.

Does nitrate produce a colored flame? Explain.

Nitrate is not responsible for the color because nitrate is in many compounds that produced different colors.

Would it matter if you did a flame test with sodium chloride, NaCl, in solid form or sodium chloride as an aqueous solution. Explain

No, nitrate does not produce a colored flame as both nitrogen and oxygen are non metals as they don't react with heat, they cannot produce colored flame

Lesson 31 pages 160-164 Question 1: How are an ionic bond and a covalent bond different? How are they Similar?

- A covalent bond is one in which nonmetal atoms share one or more pairs of electrons with one another. An ionic bond is one in which a metal atom gives up electrons to a nonmetal atom. - They both involve the bonded atoms receiving a full valence shell of eight electrons

Lesson 19 pages 93-97 Question 7: Which noble gas is closest to Sulfur, S, on the periodic table? What must happen to a Sulfur atom to have an electron arrangement similar to that of a noble gas?

- Argon, Ar - It should gain two electrons to have an electron arrangement similar to that of argon.

Lesson 19 pages 93-97 Question 6: Which noble gas is closets to Magnesium, Mg on the periodic table? What must happen to a Magnesium atom to have an electron arrangement similar to that of a noble gas?

- Neon, Ne - It should give away two valance electrons (because it is in group 2A)

Lesson 19 pages 93-97 Question 10: What charge would an arsenic, As, ion have?

-3 charge

Lesson 30 pages 156-159 Question 1: What is the HONC 1234 rule?

-Hydrogen can only have 1 bond -Oxygen can only have 2 bonds -Nitrogen can only have 3 bonds -Carbon can only have 4 bonds

Lesson 31 pages 160-164 Question 7: In your own words explain why the HONC 1234 rule works.

-Hydrogen has 1 valence electron, and it requires just one electron to complete it's duplet attain stability, similarly, O, N and C have 6, 5 and 4 valence electrons respectively. Hence, they require 2, 3, and 4 electrons to be shared by other elements to complete their respective octets. -H, O, N and C always make 1, 2, 3 and 4 electron bonding pairs. The bonding pairs may be single bonds, double bonds or triple bonds, or a combination of any of these, but the total no of bonds made by each of these element is always fixed.

Lesson 28 pgs 146-150 Question 4: Make a list of five things from home that have no smell.

-air, water, table, phone, door

Lesson 28 pgs 146-150 Question 3: Name five substances from home that do not fit into the smell categories of sweet, minty, or fishy. What new categories would you put them in?

-ammonia and bleach (chemical category) -blue cheese (pungent category) -rotting meat, sour milk (decayed category)

Lesson 22 pages 109-111 Question 5: Sodium cyanide, NaCN, contains a cyanide ion. What is the charge on the cyanide ion?

1-

Lesson 21 pages 103-108 Question 6: Give examples of 3 ionic compounds with a metal to nonmetal ratio of 1:2. Specify the total number of valence electrons for each compound. Name each compound.

1.)CaBr2,calcium bromide, 8 valence electrons 2.)MgCl2, magnesium chloride, 8 valence electrons 3.)BeF2, Beryllium fluoride, 8 valence electrons

Lesson 22 pages 109-111 Question 6: Calcium phosphate, Ca3(PO4)2, contains phosphate ions. What is the charge on a phosphate ion?

3-

Lesson 29 pgs 151-155 Question 1: What information does a structural formula provide?

A diagram or drawing that shows how the atoms in a molecule are arranged and where they are connected.

Lesson 24 pgs. 116-121 Question 2: What is an electron configuration?

A notation for keeping track of where the electrons in an atom are distributed among the shells and subshells in an atom.

Lesson 19 pages 93-97 Question 12: When chlorine gains an electron to become a chloride ion with a -1 charge, it ends up with the electron arrangement of argon. Why doesn't it become an argon atom?

Because the only thing that is changing in the atom is the number of electrons, the protons, neutrons, and atomic mass stay the same.

Lesson 33 pages 169-173 Question 3: Explain why C2H4 has fewer hydrogen atoms than C2H6.

C2H4 has fewer hydrogen atoms because the two carbon are held together by double bonds.

What evidence supports the claim that chloride, Cl^-, does not cause the flame to have a color? A.) Lithium Chloride, LiCl, and sodium chloride, NaCl, have different colors. B.) Ammonium chloride, NH4Cl, does not cause the flame to have a color. C.) Sodium chloride, NaCl and sodium nitrate, NaNO3, both produce flames with a yellow-orange color. D.) All of the above.

D.) All of the above.

Lesson 21 pages 103-108 Question 1: Explain how to use the periodic table to determine the charges on the ions.

For main group elements, the group number shows the number of valence electrons. Since metal atoms have a positive charge, we know which elements' ions have a positive charge, and since nonmetal atoms have a negative charge, we know which elements' ions have a negative charge.

Lesson 33 pages 169-173 Question 1: What is a functional group?

Lesson 33 pages 169-173 A functional group is a part of molecule and is specific group, which determines the properties and functional characteristics of molecules

Lesson 32 pages 165-168 Question 4: List 2 nonmetal elements that combine with 3 hydrogen atoms to satisfy the octet rule.

Nitrogen and Phosphorus because Nitrogen forms NH3, and phosphorus forms PH3. Both N and P have a lone pair when bonded to 3 H atoms, making a total of 8 electrons around the N or P atom. Therefore, these structures both follow the octet rule.

Lesson 32 pages 165-168 Question 1: Explain why nitrogen bonds with hydrogen to form NH3, but not NH2 or NH4. Use Lewis dot structures to support your argument. (draw diagrams on paper)

Nitrogen has 3 unpaired electrons and hydrogen has 1 unpaired electron, so 3 hydrogen and form bonds with one nitrogen, giving the nitrogen an octet of electrons and each hydrogen atom 2 electrons. (following the rule of zero charge basically)

Lesson 19 pages 93-97 Question 2: Explain what is meant by noble gas envy.

Nobel gas envy is the idea that every element wants to have atoms that are stable like the noble gases. Because of this, they give or take electrons to become stable.

Lesson 18 pages 88-92 Question 5: For main group elements, how does the number of core electrons vary across a period?

Period 2 always has 2 core electrons, period 3 always has 8 core electrons, and with the exception of Potassium, K, and Calcium, Ca, period 4 always has 28 valence electrons.

Lesson 19 pages 93-97 Question 9: List 4 ions that have the same number of electrons as argon, Ar.

S^2-, Cl-, K+, Ca^2+

Lesson 19 pages 93-97 Question 4: Give 2 similarities and 2 differences between Cl and Cl-.

Similarities... 1.) 17 protons 2.) 18 neutrons Differences... 1.) Cl- has 18 electrons and Cl has 17 electrons 2.) Cl- is known as a anion

Lesson 19 pages 93-97 Question 5: Give 2 similarities and 2 differences between Be and Be^2+.

Similarities... 1.) 4 protons 2.) Both are not negatively charged Differences... 1.) Be^2+ has electrons 2 electrons whereas Be has 4 electrons 2.) Be has a neutral charge and Be^2+ has a positive charge

Lesson 29 pgs 151-155 Question 6: Two molecules have the same molecular formula, yet one smells sweet and the other smells putrid. Explain how you think this might be possible.

The bonds are in different places

How did the flame test provide evidence that specific atoms are present in compounds?

The color of the flame produced during a flame test is a characteristic of particular metallic elements. When a compound containing one of the metallic elements is heated, its atoms emit light of a specific color.

Lesson 33 pages 169-173 Question 2: What information would you want to have to predict the smell of a compound? Explain why.

The compound's functional group because the functional group is what determines the smell of the compound. The molecular structure will help you determine the functional group of a compound.

Lesson 19 pages 93-97 Question 14: What periodic patterns do you notice for the charges on the ions?

The elements in groups 1A - 4A have positive charges that are the same as their group numbers. 5A - 7A have negative charges that are their group number minus eight. Group 8A has a neutral charge.

Lesson 21 pages 103-108 Question 2: Explain how to use the periodic table to determine the correct formulas for ionic compounds.

The group number of the main group elements tells you the number of valence electrons an atom of that element has. Also the charges on the ion is what dictates which ions come together to form bonds. Two ions will come together if their charge adds up to zero, and if this happens then you know it is a correct formula.

Explain what is responsible for the colors during a flame test.

The metals in the compound are what is responsible for the colors in the flame test.

Lesson 24 pgs. 116-121 Question 12: You should be able to figure out the identity of an atom from its electron configuration alone. Describe at least two ways you could do this.

Way 1: Add all the numbers that are present in the electron configuration. They are basically the number of electrons in the respective shells of the atom. The sum of these numbers will give the total number of electrons, which is the atomic number of the atom. From the atomic number, the element can be easily identified. (For example, lets take the electron configuration..) - 1s2 2s2 2p6 3s2 3p5 - 2+2+6+2+5 = 17 - Element with atomic number 17 is Chlorine. Way 2: The second way is by observing the last subshell in the electron configuration. Suppose it is 2s1, then simply find the 1st element in the 2nd period of the s block! (Example...) - 1s2 2s2 2p6 3s2 3p5 - Here, the last subshell is 3p5. - Now, the 3rd Period in P block is Al, Si, P, S, Cl, (Cl being the 5th.) -The element is Cl.

Predict the color of the flame for the compound sodium hydroxide, NaOH. Explain your reasoning.

Yellow-Orange because the element Na always creates that color.

Lesson 29 pgs 151-155 Question 3: If you are given a structural formula of a molecule, do you also know its molecular formula for each of the molecules?

Yes

Lesson 24 pgs. 116-121 Question 11: Write the electron configuration for each of these atoms. Then write it using the noble gas shorthand method. a.) oxygen b.) chlorine c.) iron d.) calcium e.) magnesium f.) silver g.) silicon h.) mercury

a.) Electron Configuration: 1s2 2s2 2p4 Noble Gas Shortcut: [He] 2s2 2p4 b.) Electron Configuration: 1s2 2s2 2p6 3s2 3p5 Noble Gas Shorthand: [Ne] 3s2 3p5 c.) Electron Configuration: 1s2 2s2 2p6 3s2 3p6 4s2 3d6 Noble Gas Shorthand: [Ar] 4s2 3d6 d.) Electron Configuration: 1s2 2s2 2p6 3s2 3p6 4s2 Noble Gas Shortcut: [Ar] 4s2 e.) Electron Configuration: 1s2 2s2 2p6 3s2 Noble Gas Shorthand: [Ne] 3s2 f.) Electron Configuration: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d9 Noble Gas Shorthand: [Kr] 5s2 4d9 g.) Electron Configuration: 1s2 2s2 2p6 3s2 3p2 Noble Gas Shorthand: [Ne] 3s2 3p2 h.) Electron Configuration: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 Noble Gas Shorthand: [Xe] 6s2 4f14 5d10

Lesson 20 pages 98-102 Question 5: For each of these compounds show that the charges on the ions add up to zero... a.) KBr b.) CaO c.) Li2O d.) CaCl2 e.) AlCl3

a.) KBr has 1 potassium ion with a charge +1 and 1 bromide ion with the charge -1. b.) CaO has 1 calcium ion with the charge +2 and 1 oxide ion with the charge -2. c.) Li2O has 2 Li ions with the charge +1 each and 1 oxide ion with the charge -2. d.) CaCl2 has one calcium ion with the charge +2 and 2 chloride ions each with the charge -1. e.) AlCl3 has 1 aluminum ion with the charge +3 and 3 chloride ions each with the charge -1.

Lesson 21 pages 103-108 Question 3: Which chemical formulas are consistent with the guidelines for creating ionic compounds? Explain your reasoning. a.) LiCl b.) LiCl2 c.) MgCl d.) MgCl2 e.) AlCl3

a.) LiCl is possible because the total of the charges on the ions equals zero. The lithium ion has a charge of +1 and the chloride ion has a charge of -1. b.) LiCl2 is not possible because the total of the charges on the ions equals -1. c.) MgCl is not possible because the total of the charges on the ions equals +1. Magnesium ions have the charge of +2. d.) MgCl2, is possible because the total of the charges on the ions equals zero. e.) AlCl3 is possible because the total of the charges on the ions equals zero. Aluminum ions have a charge of +3.

Lesson 28 pgs 146-150 Question 7: Predict the smells of these molecules. Explain your reasoning. a.) methyl octenoate, C9H18O2 b.) Monoethylamine, C2H7N c.) ethyl acetate, C4H8O2

a.) Sweet because it has twice the hydrogen than carbon and 2 oxygen, ends in ate b.) Fishy because it has Nitrogen, also ends in ine b.) Sweet because it has twice the hydrogen than carbon and 2 oxygen, ends in ate

Lesson 31 pages 160-164 Question 6: How many lone pairs does each of the molecules in exercise 5 have? a.) TeCl2 = ? b.) HI = ? c.) AsBr3 = ? d.) SiF4 = ? e.) F2 = ?

a.) TeCl2 = 14 b.) HI = 6 c.) AsBr3 = 20 d.) SiF4 = 24 e.) F2 = 12

Lesson 18 pages 88-92 Question 8: see hw

a.) Tin, Sn, Group 4A b.) 50 protons, because the atomic number is 50 c.) 69 neutrons, because the average atomic mass is 118.7 which rounds to 119 and 119-50=69 (subtracted protons from mass) d.) 50 electrons, because the atomic number is 50 e.) 4 valence electrons, because it is in group 4A f.) 46 core electrons, because 50-4=46 g.) Lead, Silicon, and Carbon, because they are all in the same group

What flame colors would be produced by these compounds. Explain your choices. a.) Na2CO3 b.) Ba(OH)2 c.) KOH d.) K2CO3 e.) BaO

a.) Yellow-Orange b.) Green c.) Pink-Lilac d.) Pink-Lilac e.) Green

Lesson 33 pages 169-173 Question 5: Consider a compound called hexanol. Chemists can tell from its name that it has six carbon (hex-) and it is an alcohol (-ol). a.) What is the molecular formula of hexanol? b.) Draw a possible structural formula for hexanol c.) Is the molecular formula or the structural formula more useful in determining the smell of hexanol? Explain.

a.) c6h14o b.) check doc c.) the structural formula because it shows the functional group which is how we know that the compound it actually hexanol.

Lesson 30 pages 156-159 Question 4: Is each structural formula correct according to the HONC 1234 rule? For any molecules that don't follow the HONC 1234 rule, repair the incorrect structural formula. (check book)

a.) correct b.) incorrect c.) correct d.) incorrect e.) correct

Lesson 22 pages 109-111 Question 7: Which chemical formula does not represent a possible compound with sulfate, SO4^2-? Explain your answer. a.) Na2SO4 b.) KSO4 c.) Al2(SO4)3 d.) CaSO4

b because potassium has a charge of 1+ so the charge of potassium and sulfate do not balance out

Lesson 33 pages 169-173 Question 4: Create a four-carbon molecule that is... b.) a carboxylic acid (draw on paper)

c4h8o2 (Ethyl acetate) (check book/slader)

Lesson 32 pages 165-168 Question 3: List 3 nonmetal elements that combine with only one fluorine atom to satisfy the octet rule.

fluorine, hydrogen and chlorine

Lesson 19 pages 93-97 Question 3: How many electrons, protons, and neutrons does Li+ have?

protons: 3 electrons: 2 neutrons: 3 or 4