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Chapter 1: Problem 6

In each of the following pairs, decide which is an element and which is a compound. (a) \(\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\) and \(\mathrm{Pt}\) (b) copper or copper(II) oxide (c) silicon or sand

Short Answer

Expert verified
(a) Pt(NH3)2Cl2 is a compound; Pt is an element. (b) Copper(II) oxide is a compound; copper is an element. (c) Sand is a compound; silicon is an element.

Step by step solution

01

Identifying Elements and Compounds: Pt(NH3)2Cl2 vs Pt

Platinum dichloride diamine, represented as \( \text{Pt}(\text{NH}_3)_2 \text{Cl}_2 \), is composed of one platinum atom, two ammonia molecules, and two chlorine atoms, making it a combination of different elements. Therefore, it is a compound. On the other hand, \( \text{Pt} \) represents pure platinum, which is a single type of atom, hence an element.
02

Identifying Elements and Compounds: Copper vs Copper(II) Oxide

Copper(II) oxide is a chemical compound represented as \( \text{CuO} \), which consists of copper and oxygen atoms. Since it contains more than one type of element, it is a compound. Copper alone, on the other hand, is made purely of copper atoms, making it an element.
03

Identifying Elements and Compounds: Silicon vs Sand

Silicon is a pure chemical element with the symbol \( \text{Si} \), consisting of only silicon atoms. Sand, however, is primarily composed of silicon dioxide \( \text{SiO}_2 \), which is a compound as it consists of silicon and oxygen atoms bound together.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Chemical Compounds
Chemical compounds are substances made up of two or more different types of elements. They are formed by chemical bonds that join different atoms together. This combination allows compounds to have distinct properties different from the individual elements they are composed of.
  • A common example is water (\( \text{H}_2\text{O} \)), which is a compound formed from hydrogen and oxygen.
  • Another example is sodium chloride (\( \text{NaCl} \)), a compound made from sodium and chlorine.
Chemical compounds can vary widely in their complexity:
  • Simple compounds like carbon dioxide (\( \text{CO}_2 \)) consist of only three atoms.
  • More complex compounds like proteins contain thousands of atoms.
Understanding compounds helps us grasp how elements interact to form diverse materials across the universe.
Chemical Elements
Chemical elements are pure substances consisting of only one type of atom. These elements are the basic building blocks of matter and are organized in the periodic table.
They are characterized by a specific number of protons in their atomic nuclei, known as the atomic number.
  • Examples include hydrogen (\( \text{H} \)), which is the simplest element with an atomic number of 1.
  • Iron (\( \text{Fe} \)) is another element, characterized by its metallic properties.
Each element has unique chemical and physical properties:
  • The metal copper (\( \text{Cu} \)) conducts electricity efficiently.
  • The non-metal oxygen (\( \text{O} \)) is vital for respiration.
By understanding chemical elements, we can better understand the materials around us and their interactions.
Chemical Nomenclature
Chemical nomenclature is the system used to name chemical substances. It helps scientists and students identify compounds based on their composition and structure. This system is essential for clear communication in the scientific community.
  • For compounds, the nomenclature often includes the names of the elements involved and numerical prefixes that convey how many atoms of each element are present.
  • An example is carbon monoxide (\( \text{CO} \)), indicating one carbon atom and one oxygen atom.
Naming compounds accurately is critical for avoiding confusion:
  • Copper(II) oxide (\( \text{CuO} \)) clearly indicates the oxidation state of copper.
  • For molecular compounds, the prefixes \( \ ext{di-}=2,\ \ ext{tri-}=3 \) are used to indicate the number of each type of atom.
By mastering chemical nomenclature, students can easily interpret chemical formulas and communicate their findings effectively.

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Most popular questions from this chapter

A The density of a single, small crystal can be determined by the flotation method. This method is based on the idea that if a crystal and a liquid have precisely the same density, the crystal will hang suspended in the liquid. A crystal that is more dense will sink; one that is less dense will float. If the crystal neither sinks nor floats, then the density of the crystal equals the density of the liquid. Generally, mixtures of liquids are used to get the proper density. Chlorocarbons and bromocarbons (see the list below) are often the liquids of choice. If the two liquids are similar, then volumes are usually additive and the density of the mixture relates directly to composition. (An example: \(1.0 \mathrm{mL}\) of \(\mathrm{CHCl}_{3}, d=1.4832 \mathrm{g} / \mathrm{mL},\) and 1.0 mL of \(\mathrm{CCl}_{4}, d=1.5940 \mathrm{g} / \mathrm{mL},\) when mixed, give \(2.0 \mathrm{mL}\) of a mixture with a density of \(1.5386 \mathrm{g} / \mathrm{mL} .\) The density of the mixture is the average of the values of the two individual components.) The problem: A small crystal of silicon, germanium, tin, or lead (Group 4A in the periodic table) will hang suspended in a mixture made of \(61.18 \%\) (by volume) \(\mathrm{CH}\) IBr \(_{3}\) and \(38.82 \%\) (by volume) \(\mathrm{CHCl}_{3} .\) Calculate the density and identify the element. (You will have to look up the values of the density of the elements in a manual such as the The Handbook of Chemistry and Physics in the library or in a World Wide Web site such as WebElements at, www.webelements.com.) $$\begin{array}{llll} \hline \text { Liquid } & \text { Density }(\mathrm{g} / \mathrm{mL}) & \text { Liquid } & \text { Density }(\mathrm{g} / \mathrm{mL}) \\ \hline \mathrm{CH}_{2} \mathrm{Cl}_{2} & 1.3266 & \mathrm{CH}_{2} \mathrm{Br}_{2} & 2.4970 \\ \mathrm{CH} \mathrm{Cl}_{3} & 1.4832 & \mathrm{CHBr}_{3} & 2.8899 \\ \mathrm{CCl}_{4} & 1.5940 & \mathrm{CBr}_{4} & 2.9609 \\ \hline \end{array}$$

The accepted value of the melting point of pure aspirin is \(135^{\circ} \mathrm{C} .\) Trying to verify that value, you obtain the melting points of \(134^{\circ} \mathrm{C}, 136^{\circ} \mathrm{C}, 133^{\circ} \mathrm{C},\) and \(138^{\circ} \mathrm{C}\) in four separate trials. Your partner finds melting points of \(138^{\circ} \mathrm{C}, 137^{\circ} \mathrm{C}, 138^{\circ} \mathrm{C},\) and \(138^{\circ} \mathrm{C}\) (a) Calculate the average value and percent error for you and your partner. (b) Which of you is more precise? More accurate?

A piece of copper has a mass of \(0.546 \mathrm{g} .\) Show how to set up an expression to find the volume of this piece of copper in units of liters. (Copper density \(=8.96 \mathrm{g} / \mathrm{cm}^{3} .\) )

About two centuries ago, Benjamin Franklin showed that 1 teaspoon of oil would cover about 0.5 acre of still water. If you know that \(1.0 \times 10^{4} \mathrm{m}^{2}=2.47\) acres, and that there is approximately \(5 \mathrm{cm}^{3}\) in a teaspoon, what is the thickness of the layer of oil? How might this thickness be related to the sizes of molecules?

Milk in a glass bottle was placed in the freezer compartment of a refrigerator overnight. By morning a column of frozen milk emerged from the bottle. Explain this observation.(IMAGE CAN'T COPY)
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