Two simulations that were used are below: This activity is structured as a game, wherein your challenge is to create correct ionic compound formulas by combining individual ions based on their charges. Once you correctly connect the atoms in the interactive website, a common use for that compound will be revealed. In this worksheet, you must record both the correct formula for each of the seven ionic compounds and their common uses as revealed by the interactive program. Throughout the activity, you will have the option of skipping each compound – if you choose to do this, its common use will not be revealed. You must correctly write the formulas and match the common uses.Website for first simulation: https://www.learner.org/wp-content/interactive/periodic/bondingClick “Begin” on the first page you see.For each compound name listed at the top of the interactive, choose the correct cation and anion which you think belong to the formula for that compound. For example: Sodium Chloride, click “Na+” and “Cl-“. 3. Drag one ion on top of the other until the two ions you want to connect are highlighted yellow. We recorded this info in a table. The second/last simulation:Open the following website: https://javalab.org/en/ion_model_en/Use the puzzle pieces to form the ionic compounds listed in data table 2, and then fill in data table 2 with that information. Write the formula for that compound and draw or copy and paste your completed puzzle for each ionic compound into the table. Scientific question: Why are compounds composed of integer ratios of elements?Hypothesis: If an atom ionizes to become a positive cation, then it will interact and bond with a negative anion to form an ionic bond. Outline the main idea of the paragraph. Use key words to clearly link to the scientific question. Write about what was done in the experiment to learn about the sytem and seek an answer to the scientific question. Discuss why this particular type of experiment was suitable to test the hypothesis. Include text based evidence from background research for support. Tie this experiment info back to the hypothesis. The answer to this MUST look similar to the example attached. JONICLewis dat structures were invented by a guy named Lewis. Each dot in a Lewis Structure represents avalence electron, and each atom is denoted with its atomic symbol. To draw a Lewis Structure, start withthe atomic symbol in the middle, then put dots around the symbol until all of the valence electrons areViewthe srepresented. Try to envision a box around the atom symbol and the electrons on each side of the box.The valence electrons should be drawn around the element symbol one on each side before pairing theelectrons up. The maximum number of electrons that could be on one side of a Lewis Structure is two,and the maximum number of electrons around an element symbol is eight.BackgroundTo figure out how many valence electrons each element has, use the Periodic Table. Remember, thenumber of valance electrons for Group A elements is equal to the Group A number the element is in onthe Periodic Table.- ** -* - · § ³× + Ø 18-2Lr Rf DbModeling the formationFr Ra Lof an ionic compound (and the chemical reaction that makes it) with Lewis dot structures can be done inJust 4 easy steps.AL-Step 1infoStep 2Step 3Modelinglons that form from one atom on the Periodic Table are called monatomic ions. However not all ionicbonds are formed with monatomic ions, polyatomic ions can form ionic bonds as well. The prefix poly-means many and atomic refers to atoms, so a polyatomic ion is an ion that contains more than oneatom. This differentiates polyatomic ions from monatomic ions, which contain only one atom. Examplesof monatomic ions include Na+, Fe3+, Cl-, and many, many others. We can think about polyatomic ionsby comparing them to manatomic ions. A monatomic ion is an atom that has been ionized by gaining orlosing electrons. The ion has a net charge because the total number of electrons is not balanced by thetotal number of protons in the nucleus. Thus, compared to the neutral atom, we have extra electrons-in the case of a negatively charged anion-or not enough electrons in the case of a positively chargedcation. For example, a neutral chlorine atom has an atomic number of 17, which means it has 17 protonsand 17 electrons. The neutral atom will sometimes gain an extra electron to become the chloride anion,C: Claed.After gaining an electron, the chloride anion has 17 protons and 18 electrons. Since there is one extraelectron compared to the number of protons, the lon has a net charge of 1-. Similarly, we can think of apolyatomic ion as a molecule that has been lonized by gaining or losing electrons. In a polyatomic ion,anonizedthe group of covalently bonded atoms carries a net charge because the total number of electrons in themolecule is not equal to the total number of protons in the molecule. For example, let's consider thepolyatomic ion OH-, which is known as hydroxide. It contains one oxygen atom and one hydrogen atom.We see that hydroxide has a 1-charge, meaning the lon has one more electron than protons in thenuclei of a hydrogen atom plus an oxygen atom. Polyatomic ions are everywhere! Bicarbonate ions,HCO3-, help maintain the pH level of our blood, while phosphates, PO43- are extremely important invarious metabolic processes. Being familiar with the names, charges, and formulas of the most commonpolyatomic ions will be helpful for recognizing ionic compounds and predicting their reactivity. Thefollowing table lists some of the common polyatomic lans.NH₂AmmoniumCH₂OCIOCloyCloyCloCNHCO,¹HSO¹HSO₂¹H₂POAcetateHypochloriteChloriteChloratePerchlorateCyanideHydrogenHydrogen SulfiteHydrogen PhosphateDihydrogen PhosphatePermanganateCarbonate (or Bicarbonate)conC₂0₂²CrO₂²NitriteNitriteNitrateHydroxide (signifies a Base)Cr₂O²HPO0₂²2OSOSO₂²CarbonateOxalatePO₂³PO³ChromateDichromateHydrogen PhosphatePeroxideMaONO₂¹NO₂¹OHNow that we have a reference for many of the comman palyatomic ions, let's look at how to write thechemical formulas for compounds that contain them. There are two main things to keep in mindSulfiteSulfatePhosphitePhosphate1. If a compound contains more than one polyatomic ion of the same type, we need to placeparentheses around the lon's formula before using a subscript to indicate how many ions of that typeare in the compound.2. The overall charge for the lonic compound must be neutral, which means the sum of the chargesfrom the cations and anions should add up to zero. We can use this rule to figure out the formula of anionic compound when we know the charge on the anion and the cation. This rule can also be useful fordeducing the charge of an ion when the chemical formula for the lonic compound is known.Example: Write the chemical formula for calcium hydroxide (calcium and hydroxide)Calcium is an alkaline earth metal in Group 2 on the periodic table, so it forms ions with a 2+ charge.From our table above, we know that hydroxide has the formula OH-. Because calcium needs to lose twovalence electrons to satisfy the Octet Rule, and hydroxide can only take one valence electron, we willneed two hydroxide ions to exactly cancel the 2+ charge on the Ca2+ ion. When writing out the formula,we include parentheses around OH followed by a subscript of 2, to make it clear that there are twohydroxide ions for every Ca2+ cation. Thus, the chemical formula for the compound is Ca(OH)2 To answer the scientific question, a virtual lab wasused to increase the abundance of theHydrogen-1 isotope. The virtual lab providesdata on the average atomic mass and percentabundance, something that would not be possiblein real life because it is not possible to change theabundance of Hydrogen-1 naturally. Thisexperiment is suitable to test the hypothesisbecause it provides information on the percentabundance and average atomic mass and, it allowsus to alter the abundance of Hydrogen-1. In thehypothesis, we are trying to see if an increase ofHydrogen-1 will increase the average atomicmass. The virtual simulation provides thenecessary information to test that hypothesis andsee if it is correct or incorrect.

Answered: Image /qna-images/answer/422642bd-faa6-4493-a361-8733aa70a7e9.jpg

Answered: Why are compounds composed of integer…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

Two simulations that were used are below:

This activity is structured as a game, wherein your challenge is to create correct ionic compound formulas by combining individual ions based on their charges. Once you correctly connect the atoms in the interactive website, a common use for that compound will be revealed. In this worksheet, you must record both the correct formula for each of the seven ionic compounds and their common uses as revealed by the interactive program.

Throughout the activity, you will have the option of skipping each compound – if you choose to do this, its common use will not be revealed. You must correctly write the formulas and match the common uses.

Website for first simulation: https://www.learner.org/wp-content/interactive/periodic/bonding

Click “Begin” on the first page you see.
For each compound name listed at the top of the interactive, choose the correct cation and anion which you think belong to the formula for that compound.

For example: Sodium Chloride, click “Na⁺” and “Cl^-“.

3. Drag one ion on top of the other until the two ions you want to connect are highlighted yellow. We recorded this info in a table.

The second/last simulation:

Open the following website: https://javalab.org/en/ion_model_en/

Use the puzzle pieces to form the ionic compounds listed in data table 2, and then fill in data table 2 with that information. Write the formula for that compound and draw or copy and paste your completed puzzle for each ionic compound into the table.

Scientific question:

Why are compounds composed of integer ratios of elements?

Hypothesis:

If an atom ionizes to become a positive cation, then it will interact and bond with a negative anion to form an ionic bond.

Outline the main idea of the paragraph. Use key words to clearly link to the scientific question. Write about what was done in the experiment to learn about the sytem and seek an answer to the scientific question. Discuss why this particular type of experiment was suitable to test the hypothesis. Include text based evidence from background research for support. Tie this experiment info back to the hypothesis.

The answer to this MUST look similar to the example attached.

JONIC
Lewis dat structures were invented by a guy named Lewis. Each dot in a Lewis Structure represents a
valence electron, and each atom is denoted with its atomic symbol. To draw a Lewis Structure, start with
the atomic symbol in the middle, then put dots around the symbol until all of the valence electrons are
View
the s
represented. Try to envision a box around the atom symbol and the electrons on each side of the box.
The valence electrons should be drawn around the element symbol one on each side before pairing the
electrons up. The maximum number of electrons that could be on one side of a Lewis Structure is two,
and the maximum number of electrons around an element symbol is eight.
Background
To figure out how many valence electrons each element has, use the Periodic Table. Remember, the
number of valance electrons for Group A elements is equal to the Group A number the element is in on
the Periodic Table.
- ** -* - · § ³× + Ø 18
-2
Lr Rf Db
Modeling the formation
Fr Ra L
of an ionic compound (and the chemical reaction that makes it) with Lewis dot structures can be done in
Just 4 easy steps.
AL-
Step 1
info
Step 2
Step 3
Modeling
lons that form from one atom on the Periodic Table are called monatomic ions. However not all ionic
bonds are formed with monatomic ions, polyatomic ions can form ionic bonds as well. The prefix poly-
means many and atomic refers to atoms, so a polyatomic ion is an ion that contains more than one
atom. This differentiates polyatomic ions from monatomic ions, which contain only one atom. Examples
of monatomic ions include Na+, Fe3+, Cl-, and many, many others. We can think about polyatomic ions
by comparing them to manatomic ions. A monatomic ion is an atom that has been ionized by gaining or
losing electrons. The ion has a net charge because the total number of electrons is not balanced by the
total number of protons in the nucleus. Thus, compared to the neutral atom, we have extra electrons-
in the case of a negatively charged anion-or not enough electrons in the case of a positively charged
cation. For example, a neutral chlorine atom has an atomic number of 17, which means it has 17 protons
and 17 electrons. The neutral atom will sometimes gain an extra electron to become the chloride anion,
C: Claed.
After gaining an electron, the chloride anion has 17 protons and 18 electrons. Since there is one extra
electron compared to the number of protons, the lon has a net charge of 1-. Similarly, we can think of a
polyatomic ion as a molecule that has been lonized by gaining or losing electrons. In a polyatomic ion,
anonized
the group of covalently bonded atoms carries a net charge because the total number of electrons in the
molecule is not equal to the total number of protons in the molecule. For example, let's consider the
polyatomic ion OH-, which is known as hydroxide. It contains one oxygen atom and one hydrogen atom.
We see that hydroxide has a 1-charge, meaning the lon has one more electron than protons in the
nuclei of a hydrogen atom plus an oxygen atom. Polyatomic ions are everywhere! Bicarbonate ions,
HCO3-, help maintain the pH level of our blood, while phosphates, PO43- are extremely important in
various metabolic processes. Being familiar with the names, charges, and formulas of the most common
polyatomic ions will be helpful for recognizing ionic compounds and predicting their reactivity. The
following table lists some of the common polyatomic lans.
NH₂
Ammonium
CH₂O
CIO
Cloy
Cloy
Clo
CN
HCO,¹
HSO¹
HSO₂¹
H₂PO
Acetate
Hypochlorite
Chlorite
Chlorate
Perchlorate
Cyanide
Hydrogen
Hydrogen Sulfite
Hydrogen Phosphate
Dihydrogen Phosphate
Permanganate
Carbonate (or Bicarbonate)
con
C₂0₂²
CrO₂²
Nitrite
Nitrite
Nitrate
Hydroxide (signifies a Base)
Cr₂O²
HPO
0₂²2
O
SO
SO₂²
Carbonate
Oxalate
PO₂³
PO³
Chromate
Dichromate
Hydrogen Phosphate
Peroxide
MaO
NO₂¹
NO₂¹
OH
Now that we have a reference for many of the comman palyatomic ions, let's look at how to write the
chemical formulas for compounds that contain them. There are two main things to keep in mind
Sulfite
Sulfate
Phosphite
Phosphate
1. If a compound contains more than one polyatomic ion of the same type, we need to place
parentheses around the lon's formula before using a subscript to indicate how many ions of that type
are in the compound.
2. The overall charge for the lonic compound must be neutral, which means the sum of the charges
from the cations and anions should add up to zero. We can use this rule to figure out the formula of an
ionic compound when we know the charge on the anion and the cation. This rule can also be useful for
deducing the charge of an ion when the chemical formula for the lonic compound is known.
Example: Write the chemical formula for calcium hydroxide (calcium and hydroxide)
Calcium is an alkaline earth metal in Group 2 on the periodic table, so it forms ions with a 2+ charge.
From our table above, we know that hydroxide has the formula OH-. Because calcium needs to lose two
valence electrons to satisfy the Octet Rule, and hydroxide can only take one valence electron, we will
need two hydroxide ions to exactly cancel the 2+ charge on the Ca2+ ion. When writing out the formula,
we include parentheses around OH followed by a subscript of 2, to make it clear that there are two
hydroxide ions for every Ca2+ cation. Thus, the chemical formula for the compound is Ca(OH)2

To answer the scientific question, a virtual lab was
used to increase the abundance of the
Hydrogen-1 isotope. The virtual lab provides
data on the average atomic mass and percent
abundance, something that would not be possible
in real life because it is not possible to change the
abundance of Hydrogen-1 naturally. This
experiment is suitable to test the hypothesis
because it provides information on the percent
abundance and average atomic mass and, it allows
us to alter the abundance of Hydrogen-1. In the
hypothesis, we are trying to see if an increase of
Hydrogen-1 will increase the average atomic
mass. The virtual simulation provides the
necessary information to test that hypothesis and
see if it is correct or incorrect.

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