Answered: Scientific question: Why are compounds…

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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Could someone help me?? The answer to this question must look similar to the example attached.

Back ground info:

Atoms of different elements combine with one another to form compounds. It is important to be able to explain how atoms actually come together to form these compounds or chemical bonds. One of the three types of bonds is an ionic bond which is a bond between a metal atom and a nonmetal atom, or a cation and an anion. The Octet Rule is the driving force behind ionic bond formation.

The octet rule refers to the tendency of atoms to prefer to have eight electrons in the valence shell. When atoms have fewer than eight electrons, they tend to react and form more stable compounds. When discussing the octet rule, we do not consider d or f electrons. Only the s and p electrons are involved in the octet rule, making it useful for the main group elements (elements not in the transition metal or inner-transition metal blocks); an octet in these atoms corresponds to an electron configuration ending with s²p⁶.

One way an atom can satisfy the Octet Rule is by transferring valence electrons from one atom to another. Atoms of metals tend to lose all their valence electrons, which leaves them with an octet from the next lowest principal energy level. Atoms of nonmetals tend to gain electrons in order to fill their outermost principal energy level with an octet. This transfer of electrons from a metal to a nonmetal creating ions, is how an ionic bond is formed. This bond is held together by electrostatic attraction, or the attraction between the positive and negative ions in the bond. Although the ions are charged in an ionic bond, the net result of the bond will be zero.

Scientists like to use pictures to help explain scientific phenomenon. We will learn to draw a picture to help explain how ionic bonds are formed. One way to model ionic compounds is using Bohr models similar to the ones drawn below. But, drawing out the whole Bohr model takes up a lot of space and can be time consuming to draw, so instead we make simplified little models called Lewis dot structures that have only the atomic symbol and the valence electrons.

The rest of the background info will be provided in a picture.

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.

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.

This is the actual question you will answer. The info above is info you will need to answer the question.

Cite the sources used in the study, both text and technology, noting how they advanced your understanding. Introduce the hypothesis. Overview high level results. Provide a one sentence summary of what you learned. Example of how to answer this is attached.

**Global Statement:**
*Present the scientific question to inform the audience of the goals relevant to your investigation.*

**Introduce Research:**
*Cite the resources used in the study, both text and technology, noting that they’ve advanced your understanding.*

**Thesis Statement:**
*Introduce the hypothesis you prioritized. Is your preliminary answer to the scientific question. It's what guided us to design the experiment.*

**Overview High-Level Results:**
*Provide a one-sentence summary of what you learned from the study.*

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The research and experimentation conducted in this lab help answer the following scientific question, “How does the percent abundance of isotopes affect the average atomic mass reported for a specific element?” A supplied text and the Isotopes and Atomic Mass simulation from PhET Interactive Simulations were relied on to collect background research and data to answer this scientific question. Furthermore, the information gathered with the labs aids in figuring out if the following hypothesis was accurate, “If I increase the percent abundance of the hydrogen-1 isotope using a computer simulation (since percent abundances are natural and cannot actually be changed), then the average atomic mass of the hydrogen element will also increase.” The experimental data demonstrated that, as the abundance of hydrogen-1 isotope increases, the average atomic mass of the hydrogen DID NOT increase. Instead, it decreased. More specifically, it was found that the average atomic mass will be similar to the mass number of the most abundant isotope.

**Background Info: Valence Electrons and Lewis Dot Structures**

**Lewis Dot Structures:**
Lewis dot structures were invented by a chemist named Lewis. Each dot in a Lewis structure represents a valence electron, which is located on the outermost shell of an atom. To draw a Lewis structure:

1. Place the atomic symbol in the center.
2. Distribute the valence electrons as dots around the symbol, using no more than one dot on each side before pairing.

The maximum number of electron pairs that can surround an element symbol is four, allowing for up to eight electrons in total (octet rule).

To determine the number of valence electrons for an element, use the Periodic Table. For Group A elements, the number of valence electrons equals the group number.

**Periodic Table:**
A color-coded periodic table showing groups 1A to 8A highlights the number of valence electrons for elements in each group. This periodic table is a useful reference for determining valence electrons and drawing Lewis dot structures.

**Modeling Ionic Bonds in Lewis Dot Structures:**

**Steps to Model Ionic Bonds:**
1. **Step 1:** Begin with individual atoms, like Aluminum (Al) and Chlorine (Cl), each with their valence electrons represented by dot structures.
2. **Step 2:** Show the transfer of electrons, where Al loses electrons and Cl gains electrons.
3. **Step 3:** Result in the formation of cations (Al^3+) and anions (Cl^-).

Ions formed from single atoms are called monatomic ions. Ions from multiple atoms are polyatomic ions. For example, Chlorine can gain an electron to become Cl^-, showing a chloride ion with a 1- charge.

**Explanation of Ionic Reactions Using Chlorine and Aluminum:**
When chlorine gains an electron from aluminum, it results in Cl^- while aluminum becomes Al^3+ after losing three electrons. The ionic compound formed shows the balance of charges with aluminum cations and chloride anions.

**Common Polyatomic Ions Table:**
Includes ions like NH₄⁺ (Ammonium), C₂H₃O₂⁻ (Acetate), NO₃⁻ (Nitrate), SO₄²⁻ (Sulfate), and PO₄³⁻ (Phosphate). Knowing these ions helps in predicting reactivity and writing chemical formulas.

**Writing Chemical Formulas with Poly

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Scientific question: Why are compounds composed of integer ratios of elements?