Lab Report 2 Bhakti Patel PDF

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Title of Lab CHEM 1041 Bhakti Patel

IntroductionFor this experiment there are many objectives that are going to be present for us such while we are conducting our experiment. It helps us distinguish between what is molecular compound and ionic compounds. It also helps us interpret the formulas and names all the polyatomic ions, molecular

compounds, as well as ionic compounds, and the acids. This experiment would help us learn rules of converting the names of various compounds to their formulas. This experiment is separated into two different exercises.

Exercise #1- Preparation for Naming Ionic and Molecular Compounds The materials needed for this exercise are some colored pencils, an access to printer, flashcards, and a pen/pencil. For Data Table 1 Firstly, I was asked to get a printed copy of the periodic table that is provided in the background of the experiment. With the help of the periodic table I was required to color all the groups of elements ( which includes metals, nonmetals, partial metals, etc.) and color the periodic table accordingly. I was also instructed to create flashcards of the common polyatomic ions that is provided in Table 2 of the Background pages, the flashcards had to give the name of each element’s ion, formula, and the charge that each one possessed. I was able to place all the polyatomic ions as they varied in their oxidation state on the same flashcard. After I completed the flashcards, I even created the cards for the strong acids that is provided in Table 3 and the diatomic atoms in Table 4. The flashcards for the acids and diatomic atoms only required for their names and formulas. After getting done with the flashcards and coloring the periodic table I took pictures of them by using my phone and sending them to my laptop. After receiving them on my laptop, I resized the pictures and then sort them in Data Table 1 according to the slots that they belonged in. Data Table 1 can be found below. Document

Photo

1

Colored Periodic Table

2

Polyatomic Ion

Note

3

Strong Acid Note Card

Diatomic Element Note Card

4

Exercise #2- Naming Ionic and Molecular Compounds The only materials that were required for this exercise were flashcards and periodic table that were created for our first exercise. Data Table 2 It provides the formulas for 20 different kinds of binary compounds. I was asked to regulate whether these compounds were ionic or molecular and was asked to provide the names of each compound. I figured out whether these compounds were ionic or molecular by perceiving the elements that were present within them. If any of the compounds possessed a metal cation and a nonmetal anion, then I considered them as ionic, but if they possessed to two nonmetals then I considered them as molecular. After knowing the type of compound, I named them. If the compound was ionic and it did not possess a transition with any variable charge, then I had to place the name of the metal followed by the name of the nonmetal by placing the suffix “-ide” with it. If the compound was ionic and if it had a transition metal with a variable charge, then I had to be placed a roman numeral that represented the charge. This would result in the sum of the charges of the compound being 0. We know that there are naming rules for the molecular compounds, So I had to manually list the elements in the order presented in the formula and add prefixes to each element by illustrating the number of atoms of that particular element in the compound. If the first element had a prefix “mono- “, it could be released, and similarly to the 5

way ionic compound names end like molecular compounds end with the last element ending with the suffix “-ide”. I recorded my findings for the types of compounds and the names in Data Table which are found below. #

Formula

Molecular or Ionic Compound?

Compound Name

1

B2O3

Molecular

Diboron Trioxide

2

N2 O

Molecular

Dinitrogen oxide

3

LiCl

Ionic

Lithium chloride

4

N2O4

Molecular

Dinitrogen tetroxide

5

SF4

Molecular

Sulfur tetrafluoride

6

BrF3

Molecular

Bromine trifluoride

7

AlBr3

Ionic

Aluminum bromide

8

SnF2

Ionic

Tin(II) fluoride

9

SiCl4

Molecular

Silicon tetrachloride

10

H2O2

Molecular

Dihydrogen dioxide

11

NaCl

Ionic

Sodium chloride

12

TiCl3

Ionic

Titanium(III) chloride

13

SiO2

Molecular

Silicon dioxide

14

Al2S3

Ionic

Aluminum sulfide

15

CCl4

Molecular

Carbon tetrachloride

16

CuF2

Ionic

Copper(II) fluoride

17

SF6

Molecular

Sulfur hexafluoride

18

P4S3

Molecular

Tetraphosphorous trisulfide

19

Xe3F4

Molecular

Trixenon tetrafluoride

20

PtCl2

Ionic

Platinum(II) chloride

For Data Table 3 I was given the names of some binary compounds and was asked to give the type of compound that each one of them are and the formula for each. I considered the rules for naming the compounds and used my information on how to apply those rules to regulate if each of them were either molecular or ionic and note down their formulas. However, with ionic compounds the names don’t give the number of atoms per each element present, so we need to determine the charges of each element and then place the correct number of each element that is needed to guarantee the sum of charges is 0. I even provided my findings in Data Table 3 which is given below. #

Compound Name

Molecular or Ionic Compound?

Formula

1

Tribromine octoxide

Molecular

Br3O8

2

Lithium selenide

Ionic

Li2Sn

6

#

Compound Name

Molecular or Ionic Compound?

Formula

3

Iodine monochloride

Molecular

ICl

4

Nitrogen monoxide

Molecular

NO

5

Iron(II) sulfide

Ionic

FeS

6

Hydrogen chloride

Molecular

HCl

7

Diboron hexahydride

Molecular

B 2 H6

8

Barium iodide

Ionic

BaI2

9

Cadmium sulfide

Ionic

CdS

10

Bromine trichloride

Molecular

BrCl3

11

Nitrogen trihydride

Molecular

NH3

12

Molybdenum(VI) fluoride

Ionic

MoF4

13

Carbon tetrabromide

Molecular

CBr4

14

Sulfur trioxide

Molecular

SO3

15

Lead(II) chloride

Ionic

PbCl2

16

Iodine hexafluoride

Molecular

IF6

17

Tetraphosphorus decasulfide

Molecular

P4S10

18

Dichlorine trioxide

Molecular

Cl2O3

19

Potassium chloride

Ionic

KCl

20

Calcium oxide

Ionic

CaO

Data Table 4 gives the formulas of polyatomic ions and acids and askes we students to give the name of the compounds. To start I considered if the formula signified a polyatomic ion or an acid. For the formulas of polyatomic ions, I considered the periodic table to determine if the metal cation had any fixed or variable charges. I used the flashcards I had made before for my exercise 1 to determine the ion. Then I placed the name of the metal cation in front of the named ions, if the metal was a transition metals then I made sure to place the suitable roman numeral along with it. However, if the ion look like an ion found the flashcard, but if they had a different oxidation state, then I had to change the suffix and prefix accordingly. If the compound was an acid, then I am supposed to know if it was a oxoacids or binary acid. If the acid was binary, I have to place “hydro- “, in front followed by the second element then place “acid” behind it. However, the acid was an oxoacid then it does not contain the “hydro- “, and I had to know if there were any prefixes or suffixes after looking at the anion. I know Oxoacids also end with “acid” at the back of their name. I have recorded all the names of the compounds in Data Table given below. #

Formula

Name

1

SO4

2-

Sulfate

2

SnCl4

Tin(IV) chloride

7

#

Formula

Name

3

ClO2-

Chlorite

4

H3PO4

Phosphoric Acid

5

Cu3(PO4)2

Copper(II) Phosphate

6

FeSO4

Iron(II) sulfate

7

NH4Cl

Ammonium Chloride

8

HClO4 (aq)

Perchloric acid

9

PO43-

Phosphate

10

K2SO3

Potassium Sulfite

11

MnO2

Manganite

12

Ca3(PO4)2

Calcium phosphate

13

NaOH

Sodium hydroxide

14

HCl (aq)

Hydrochloric acid

15

HNO3 (aq)

Nitric acid

16

FeSO3

Iron(II) Sulfite

17

WO3

Tungsten(VI) oxide

18

H2CO3

Carbonic Acid

19

KMnO4

Potassium Permanganate

20

H2S (aq)

Hydrosulfric acid

This table is similar to the above, but instead of the formulas it states the names of the polyatomic ions and acids and inquires me to deliver the formulas for these compounds. I used my knowledge of the rules provided above the top data to help me in consider the formulas for each name that are given. I was also essential for me to use the flascards to find the charges of the ions based on the formulas to determine how many of cation and anion was needed in the formulas so that it could give a neutral charge. I recorded my all my data below: #

Name

Formula

1

Potassium nitrate

KNO3

2

Carbonate ion

CO3

3

Dihydrogen phosphate

H2PO3

4

Hypochlorous acid

HClO

5

Hydrogen cyanide

HCN

6

Cobalt(III) sulfite

Co2(SO3)3

7

Permanganic acid

HMnO4

8

Magnesium hypochlorite

Mg(ClO)2

8

#

Name

Formula

9

Hydroiodic acid

HI

10

Titanium(IV) nitrate

Ti(NO3)4

11

Silver chromate

Ag2CrO4

12

Nickel(II) phosphate

Ni3(PO4)2

13

Sulfuric acid

H2SO4

14

Magnesium nitride

Mg3N2

15

Hydrobromic acid

HBr

16

Ammonium ion

NH4

17

Lithium hypochlorite

LiClO

18

Nitrous acid

HNO2

19

Barium hydrogen sulfite

Ba(HSO3)2

20

Hydrofluoric acid

HF

While I was conducting this exercise, I was given few questions that I was supposed to answer for. The First had to determine the effect oh H+ to polyatomic ion phosphate. I realized it increase the charge by 1 because of +1 hydrogen charge. Therefore, the new compound formed is Hydrogen Phosphate. Secondly, I was supposed to consider the metals tat posses the fixed charged of +3 which were Group IIIA and the Period 3 that considered aluminum. Thirdly, we got to consider the difference between molecular and Ionic compounds. I learned ionic compounds contain metallic cations and nonmetal anion, whereas molecular compounds contains about two nonmetals,

ConclusionThis experiment has significantly advanced my understanding of the differences between molecular and ionic compounds both in the naming conventions and the formulas themselves. I also now possess a better understanding of acids and polyatomic ions because of these exercises, specifically Exercise #2 Data Tables #4 and #5. I feel like this experiment has helped further my growth with understanding these different types of compounds.

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