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chemistry and chemical reactivity

Questions and Answers of Chemistry And Chemical Reactivity

Give a formula for each of the following compounds:(a) A soluble compound containing the bromide ion(b) An insoluble hydroxide(c) An insoluble carbonate(d) A soluble nitrate-containing compound(e) A
Classify each of the following reactions as a precipitation, acid–base, or gas-forming reaction. Show states for the products (s, ℓ, g, aq), and then balance the completed equation. Write the net
Classify each of the following reactions as a precipitation, acid–base, or gas-forming reaction. Show states for the products (s, ℓ, g, aq), and then balance the completed equation. Write the net
Balance each of the following equations, and classify them as precipitation, acid–base, gas-forming, or oxidation–reduction reactions. Show states for reactants and products (s, ℓ, g, aq). (a)
Complete and balance the equations below, and classify them as precipitation, acid–base, gasforming, or oxidation–reduction reactions. Show states for reactants and products (s, ℓ, g, aq).
The products formed in several reactions are given below. Identify the reactants (labeled x and y) and write the complete balanced equation for each reaction. (a) x + y → H₂O(l) +
The products formed in several reactions are given below. Identify the reactants (labeled x and y) and write the complete balanced equation for each reaction. (a) x + y → (NH4)2SO4(aq) (b) x +
Indicate which of the following copper(II) salts are soluble in water and which are insoluble: Cu(NO3)2, CUCO3, Cu3(PO4)2, CuCl₂.
Give the formula for each of the following compounds:(a) A soluble compound containing the acetate ion(b) An insoluble sulfide(c) A soluble hydroxide(d) An insoluble chloride(e) A strong Brønsted
Write the net ionic equation and identify the spectator ion or ions in the reaction of nitric acid and magnesium hydroxide. What type of reaction is this? 2 H3O+ (aq) + 2 NO3(aq) + Mg(OH)₂(s)
Name two anions that combine with Al3+ ion to produce water-soluble compounds.
Identify and name the water-insoluble product in each reaction and write the net ionic equation: (a) CuCl₂(aq) + H₂S(aq) → CuS + 2 HCI (b) CaCl₂(aq) + K₂CO3(aq) → 2 KCl + CaCO3 (c)
Bromine is obtained from sea water by the following redox reaction(a) What has been oxidized? What has been reduced?(b) Identify the oxidizing and reducing agents. Cl₂(g) + 2 NaBr(aq) → 2
Identify each of the following substances as a likely oxidizing or reducing agent: HNO3, Na, Cl2, O2, KMnO4.
The Tollen’s test for the presence of reducing sugars (say, in a urine sample) involves treating the sample with silver ions in aqueous ammonia. The result is the formation of a silver mirror
The mineral dolomite contains magnesium carbonate. This reacts with hydrochloric acid.(a) Write the net ionic equation for this reaction and identify the spectator ions.(b) What type of reaction is
Aqueous solutions of ammonium sulfide, (NH4)2S, and Hg(NO3)2 react to produce HgS and NH4NO3.(a) Write the overall, balanced equation for the reaction. Indicate the state (s, aq) for each
Balance equations for these reactions that occur in aqueous solution, and then classify each as a precipitation, acid–base, or gas-forming reaction. Show states for the products (s, ℓ, g, aq),
Identify the primary species (atoms, molecules, or ions) present in an aqueous solution of each of the following compounds. Decide which species are Brønsted acids or bases and whether they are
(a) Name and give formulas for two water-soluble compounds containing the Cu2+ ion. Name two water-insoluble compounds containing the Cu2+ ion.(b) Name and give formulas for two water-soluble
You are given mixtures containing the following compounds. Which compound in each pair could be separated by stirring the solid mixture with water?(a) NaOH and Ca(OH)2(b) MgCl2 and MgF2(c) AgI and
Identify, from each list below, the compound or compounds that will dissolve in water to give a solution that strongly conducts electricity.(a) CuCO3, Cu(OH)2, CuCl2, CuO(b) HCl, H2C2O4, H3PO4, H2SO4
Identify, from each list below, the compound or compounds that will dissolve in water to give a solution that is only a very weak conductor of electricity.(a) NH3, NaOH, Ba(OH)2, Fe(OH)3(b) CH3CO2H,
If you have “silverware” in your home, you know it tarnishes easily. Tarnish is from the oxidation of silver in the presence of sulfur-containing compounds (in the atmosphere or in your food) to
Write net ionic equations for the following reactions: (a) The reaction of acetic acid, a weak acid, and Sr(OH)2(aq).(b) The reaction of zinc and hydrochloric acid to form zinc(II) chloride and
The following reaction can be used to prepare iodine in the laboratory. (a) Determine the oxidation number of each atom in the equation. (b) What is the oxidizing agent, and what has been oxidized?
Gas evolution was observed when a solution of Na2S was treated with acid. The gas was bubbled into a solution containing Pb(NO3)2, and a black precipitate formed. Write net ionic equations for the
Heating HI(g) at 425°C causes some of this compound to decompose, forming H2(g) and I2(g). Eventually, the amounts of the three species do not change further; the system has reached equilibrium. (At
Suppose you wish to prepare a sample of magnesium chloride. One way to do this is to use an acid–base reaction, the reaction of magnesium hydroxide with hydrochloric acid.When the reaction is
Suggest a laboratory method for preparing barium phosphate. (See Study Question 97 for a way to approach this question.)Data given in Question 97Describe how to prepare BaSO4, barium sulfate, by(a) A
There are many ionic compounds that dissolve in water to a very small extent. One example is lead(II) chloride. When it dissolves an equilibrium is established between the solid salt and its
Most naturally occurring acids are weak acids. Lactic acid is one example.If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest
You want to prepare barium chloride, BaCl2, using an exchange reaction of some type. To do so, you have the following reagents from which to select the reactants: BaSO4, BaBr2, BaCO3, Ba(OH)2, HCl,
Describe how to prepare BaSO4, barium sulfate, by(a) A precipitation reaction and(b) A gas-forming reaction. The available starting materials are BaCl2, BaCO3, Ba(OH)2, H2SO4, and Na2SO4. Write
A common method for analyzing for the nickel content of a sample is to use a precipitation reaction. Adding the organic compound dimethylglyoxime to a solution containing Ni2+ ions precipitates a red
Describe how to prepare zinc chloride by (a) An acid–base reaction, (b) A gas-forming reaction, and(c) An oxidation–reduction reaction. The available starting materials are ZnCO3, HCl, Cl2,
The presence of arsenic in a sample that may also contain another Group 5A element, antimony, can be confirmed by first precipitating the As3+ and Sb3+ ions as yellow solid As2S3 and orange solid
The lanthanide elements react with oxygen to give, generally, compounds of the type Ln2O3 (where Ln stands for a lanthanide element). However, there are interesting exceptions, such as a common oxide
You have a bottle of solid barium hydroxide and some dilute sulfuric acid. You place some of the barium hydroxide in water and slowly add sulfuric acid to the mixture. While adding the sulfuric acid,
What are the three fundamental particles from which atoms are built? What are their electric charges? Which of these particles constitute the nucleus of an atom? Which is the least massive particle
An atom has a very small nucleus surrounded by an electron “cloud.” Figure 2.1 represents the nucleus with a diameter of about 2 mm and describes the electron cloud as extending over 200 m. If
Define mass number. What is the difference between mass number and atomic mass?
A gold atom has a radius of 145 pm. If you could string gold atoms like beads on a thread, how many atoms would you need to have a necklace 36 cm long?
How many electrons, protons, and neutrons are there in each of the following atoms?(a). Magnesium-24, 24Mg(b). Tin-119, 119Sn(c). Thorium-232, 232Th(d). Carbon-13, 13C(e). Copper-63, 63Cu(f).
Give the complete symbol including atomic number and mass number, for each of the following atoms: (a). Magnesium with 15 neutrons, (b). Titanium with 26 neutrons, and (c). Zinc with 32 neutrons.
Give the complete symbol including atomic number and mass number, of (a). A nickel atom with 31 neutrons, (b). A plutonium atom with 150 neutrons, and (c). A tungsten atom with 110 neutrons. (x7)
In 1886 Eugene Goldstein observed positively charged particles moving in the opposite direction to electrons in a cathode ray tube (illustrated below). From their mass, he concluded that these
Marie Curie was born in Poland but studied and carried out her research in Paris. In 1903, she shared the Nobel Prize in Physics with H. Becquerel and her husband Pierre for their discovery of
(a). The synthetic radioactive element technetium is used in many medical studies. Give the number of electrons, protons, and neutrons in an atom of technetium-99. (b). Radioactive americium-241 is
From cathode ray experiments, J. J. Thomson estimated that the mass of an electron was “about a thousandth” of the mass of a proton. How accurate is that estimate? Calculate the ratio of the mass
Early in the 1800s John Dalton proposed that an atom was a “solid, massy, hard, impenetrable, moveable particle.” Critique this description. How does this description misrepresent atomic
Which of the following are isotopes of element X, the atomic number for which is 9:and 19X, 20X, X, 9 184
The mass of an 16O atom is 15.995 u. What is its mass relative to the mass of an atom of 12C?
What is the mass of one 16O atom, in grams? (The mass of an 16O atom is 15.995 u.)
Thallium has two stable isotopes, 203Tl and 205Tl. Knowing that the atomic weight of thallium is 204.4, which isotope is the more abundant of the two? EXAMPLE 2.2 Calculating Atomic Weight from
Cobalt has three radioactive isotopes used in medical studies. Atoms of these isotopes have 30, 31, and 33 neutrons, respectively. Give the complete symbol for each of these isotopes
Naturally occurring silver exists as two isotopes having mass numbers 107 and 109. How many protons, neutrons, and electrons are there in each of these isotopes?
Name and describe the composition of the three hydrogen isotopes.
Verify that the atomic weight of lithium is 6.94, given the following information: 6Li, mass = 6.015121 u; percent abundance = 7.50% 7Li, mass = 7.016003 u; percent abundance = 92.50% EXAMPLE
Verify that the atomic weight of magnesium is 24.31, given the following information: 24Mg, mass = 23.985042 u; percent abundance = 78.99% 25Mg, mass = 24.985837 u; percent abundance =
Gallium has two naturally occurring isotopes, 69Ga and 71Ga, with masses of 68.9257 u and 70.9249 u, respectively. Calculate the percent abundances of these isotopes of gallium. EXAMPLE
Europium has two stable isotopes, 151Eu and 153Eu, with masses of 150.9197 u and 152.9212 u, respectively. Calculate the percent abundances of these isotopes of europium. EXAMPLE 2.2 Calculating
Titanium and thallium have symbols that are easily confused with each other. Give the symbol, atomic number, atomic weight, and group and period number of each element. Are they metals, metalloids,
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,
How many periods of the periodic table have 8 elements, how many have 18 elements, and how many have 32 elements?
How many elements occur in the seventh period? What is the name given to the majority of these elements, and what well-known property characterizes them?
Select answers to the questions listed below from the following list of elements whose symbols start with the letter C: C, Ca, Cr, Co, Cd, Cl, Cs, Ce, Cm, Cu, and Cf. (You should expect to use some
Give the name and chemical symbol for the following. (a). A nonmetal in the second period (b). An alkali metal in the fifth period (c). The third-period halogen (d). An element that is a gas at
Classify the following elements as metals, metalloids, or nonmetals: N, Na, Ni, Ne, and Np.
Here are symbols for five of the seven elements whose names begin with the letter B: B, Ba, Bk, Bi, and Br. Match each symbol with one of the descriptions below. (a). A radioactive element (b). A
A model of nitric acid is illustrated here. Write the molecular formula for nitric acid, and draw the structural formula. Describe the structure of the molecule. Is it flat? That is, are all the
A model of the amino acid asparagine is illustrated here. Write the molecular formula for the compound, and draw its structural formula. Asparagine, an amino acid
What is the charge on the common monatomic ions of the following elements? (a). Magnesium (b). Zinc (c). Nickel (d). Gallium
What is the charge on the common monatomic ions of the following elements? (a). Selenium (b). Fluorine (c). Iron (d). Nitrogen
When a potassium atom becomes a monatomic ion, how many electrons does it lose or gain? What noble gas atom has the same number of electrons as a potassium ion?
What are the charges on the ions in an ionic compound containing the elements barium and bromine? Write the formula for the compound.
Give the formula and the number of each ion that makes up each of the following compounds: (a). K2S(b). CoSO4 (c). KMnO4 (d). (NH4)3PO4(e). Ca(ClO)2 (f). NaCH3CO2
Give the formula and the number of each ion that makes up each of the following compounds: (a). Mg(CH3CO2)2 (b). Al(OH)3 (c). CuCO3 (d). Ti(SO4)2 (e). KH2PO4 (f). CaHPO4
When oxygen and sulfur atoms become monatomic ions, how many electrons does each lose or gain? Which noble gas atom has the same number of electrons as an oxide ion? Which noble gas atom has the same
Cobalt forms Co2+ and Co3+ ions. Write the formulas for the two cobalt oxides formed by these transition metal ions.
Platinum is a transition element and forms Pt2+ and Pt4+ ions. Write the formulas for the compounds of each of these ions with (a). Chloride ions and (b). Sulfide ions.
Which of the following are correct formulas for ionic compounds? For those that are not, give the correct formula. (a) AlCl2 (b) KF2 (c) Ga2O3 (d) MgS
What are the charges of the ions in an ionic compound containing cobalt(III) and fluoride ions? Write the formula for the compound.
Name each of the following ionic compounds: (a). K2S (b). CoSO4 (c). (NH4)3PO4 (d). Ca(ClO)2
Give the formula for each of the following ionic compounds: (a) ammonium carbonate (b). Calcium iodide (c). Copper(II) bromide (d). Aluminum phosphate (e). Silver(I) acetate
Which of the following are correct formulas for ionic compounds? For those that are not, give the correct formula. (a). Ca2O (b). SrBr2 (c). Fe2O5 (d). Li2O
Write the formulas for the four ionic compounds that can be made by combining each of the cations Na+ and Ba2+ with the anions CO32− and I−. Name each of the compounds.
Name each of the following ionic compounds: (a). Ca(CH3CO2)2 (b). Ni3(PO4)2 (c). Al(OH)3 (d). KH2PO4
Give the formula for each of the following ionic compounds: (a). Calcium hydrogen carbonate(b). Potassium permanganate(c). Magnesium perchlorate(d). Potassium hydrogen phosphate(e). Sodium sulfite
Write the formulas for the four ionic compounds that can be made by combining the cations Mg2+ and Fe3+ with the anions PO43− and NO3 −. Name each compound formed.
Sodium ions, Na+, form ionic compounds with fluoride ions, F−, and iodide ions, I−. The radii of these ions are as follows: Na+ = 116 pm; F− = 119 pm; and I− = 206 pm. In which ionic
Name each of the following binary, nonionic compounds: (a). NF3 (b). HI (c). BI3 (d). PF5
Consider the two ionic compounds NaCl and CaO. In which compound are the cation–anion attractive forces stronger? Explain your answer.
Give the formula for each of the following compounds: (a). Sulfur dichloride (b). Dinitrogen pentaoxide (c). Silicon tetrachloride (d). Diboron trioxide (commonly called boric oxide)
Name each of the following binary, nonionic compounds: (a). N2O5 (b). P4S3 (c). OF2 (d). XeF4
Give the formula for each of the following compounds: (a). Bromine trifluoride (b). Xenon difluoride (c). Hydrazine (d). Diphosphorus tetrafluoride (e). Butane
Calculate the mass, in grams, of each the following:(a). 2.5 mol of aluminum(b). 1.25 × 10−3 mol of iron(c). 0.015 mol of calcium(d). 653 mol of neon
Calculate the mass, in grams, of each the following:(a). 4.24 mol of gold(b). 15.6 mol of He(c). 0.063 mol of platinum(d). 3.63 × 10−4 mol of Pu
Calculate the amount (moles) represented by each of the following:(a). 127.08 g of Cu(b). 0.012 g of lithium(c). 5.0 mg of americium(d). 6.75 g of Al
Calculate the amount (moles) represented by each of the following: (a). 16.0 g of Na(b). 0.876 g of tin(c). 0.0034 g of platinum(d). 0.983 g of Xe

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