Ular) react together to produce newThe first step in writing balanced chemical reactions is identifying the substances in the reaction andlabeling them as elements, molecular compounds or ionic compounds. Based on the type of substance it is, youthen write the correct formula from the given name.Element: a single type of atom or a diatomic element. Recognized in the description as a single elementname by itself. Elements are always neutral (they have no charge). Check if a diatomic element.Molecular compound: made of two nonmetal atoms. Greek prefixes in the name indicate the number ofeach type of atom in the formula.lonic compound: made of a cation and anion. Recognized because they start with a metal or ammonium.Need the charges of the ions to determine the formula of the neutral compound.For each chemical name below label it as an element (E), molecular (M), or ionic (I) and then write the correctformula for the substance on the line next to it.1. Aluminum reacts with sulfur to produce aluminum sulfide.EMI aluminum:EMI sulfur:2. Zinc reacts with oxygen to produce zinc oxide.EMI zinc:E MI oxygen:EMI oxygen:EMI aluminum sulfide:3. Nitrogen reacts with oxygen to produce dinitrogen monoxide gas.EM I nitrogen:EMI zinc oxide:EMI copper:EMI silver nitrate:E MI dinitrogen monoxide:4. Copper reacts with aqueous silver nitrate to produce aqueous copper(II) nitrate and silver.E MI copper(II) nitrate:EMI silver:

we have to write the correct formula of the given species and identify if it is element, ionic or…

For each chemical name below label it as an element (E), molecular (M), or ionic (1) and then write the correct formula for the substance on the line next to it. 1. Aluminum reacts with sulfur to produce aluminum sulfide. MI aluminum: MI sulfur: E E 2. Zinc reacts with oxygen to produce zinc oxide. E MI zinc: E MI oxygen: E MI aluminum sulfide: E MI zinc oxide: 3. Nitrogen reacts with oxygen to produce dinitrogen monoxide gas. E MI nitrogen: E MI oxygen: E MI dinitrogen monoxide: 4. Copper reacts with aqueous silver nitrate to produce aqueous copper(II) nitrate and silver. E MI copper: E MI copper(II) nitrate: E MI silver nitrate: E MI silver:

For each chemical name below label it as an element (E), molecular (M), or ionic (1) and then write the correct formula for the substance on the line next to it. 1. Aluminum reacts with sulfur to produce aluminum sulfide. MI aluminum: MI sulfur: E E 2. Zinc reacts with oxygen to produce zinc oxide. E MI zinc: E MI oxygen: E MI aluminum sulfide: E MI zinc oxide: 3. Nitrogen reacts with oxygen to produce dinitrogen monoxide gas. E MI nitrogen: E MI oxygen: E MI dinitrogen monoxide: 4. Copper reacts with aqueous silver nitrate to produce aqueous copper(II) nitrate and silver. E MI copper: E MI copper(II) nitrate: E MI silver nitrate: E MI silver:

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 69AP

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Similar questions

Which of the following statements is/are always true? Never true? Usually true? (a) Compounds containing chlorine can be either molecular or ionic. (b) An ionic compound always has at least one metal. (c) When an element in a molecule has a di prefix, it means that the element has a +2 charge.
These questions concern the work of J. J. Thomson: From Thomson’s work, which particles do you think he would feel are most important in the formation of compounds (chemical changes) and why? Of the remaining two subatomic particles, which do you place second in importance for forming compounds and why? Come up with three models that explain Thomson’s findings and evaluate them. To be complete you should include Thomson’s findings.
Consider the chemical reaction as depicted below. Label as much as you can using the terms atom, molecule, element, compound, ionic, gas, and solid.
The following chart shows a general decline in abundance with increasing mass among the first 30 elements. The decline continues beyond zinc. Notice that the scale on the vertical axis is logarithmic, that is, it progresses in powers of 10. The abundance of nitrogen, for example, is 1/10,000 (1/104) of the abundance of hydrogen. All abundances are plotted as the number of atoms per 102 atoms of H. (The fact that the abundances of Li, Be, and B, as well as those of the elements near Fe, do not follow the general decline is a consequence of the way that elements are synthesized in stars.) (a) What is the most abundant main group metal? (b) What is the most abundant nonmetal? (c) What is the most abundant metalloid? (d) Which of the transition elements is most abundant? (e) Which halogens are included on this plot, and which is the most abundant?
In Groups 4A-6A, there are several elements whose symbols begin with S. Name these elements, and for each one give its symbol, atomic number, group number, and period. Describe each as a metal, metalloid, or nonmetal.
Draw a formula for each of the following molecules using circular symbols of your choice to represent atoms: a. A diatomic molecule of an element b. A diatomic molecule of a compound c. A triatomic molecule of an element d. A molecule of a compound containing one atom of one element and four atoms of another element
Two basic laws of chemistry are the law of conservation of mass and the law of constant composition. Which of these laws (if any) do the following statements illustrate? (a) Lavoisier found that when mercury(ll) oxide, HgO, decomposes, the total mass of mercury (Hg) and oxygen formed equals the mass of mercury(ll) oxide decomposed. (b) Analysis of the calcium carbonate found in the marble mined in Carrara, Italy, and in the stalactites of the Carlsbad Caverns in New Mexico gives the same value for the percentage of calcium in calcium carbonate. (c) Hydrogen occurs as a mixture of two isotopes, one of which is twice as heavy as the other.
The mass spectrum of nitrogen dioxide is illustrated here. (a) Identify the cations present for each of the four peaks in the mass spectrum. (b) Does the mass spectrum provide evidence that the two oxygen atoms are attached to a central nitrogen atom (ONO), or that an oxygen atom is at the center (NOO)? Explain.
What is acompound? What are compounds composed of? What is true about the composition of a compound, no matter where we happen to find the compound?
In a neutron star, gravity causes the electrons to combine with protons to form neutrons. A typical neutron star has a mass half that of the sun, compressed into a sphere of radius 20 km. If such a neutron star contains 6.01056 neutrons, calculate its density in grams per cubic centimeter. Compare this with the density inside a 232Th nucleus, in which 142 neutrons and 90 protons occupy a sphere of radius 9.11013cm . Take the mass of a neutron to be 1.6751024g and that of a proton to be 1.6731024g .