Concept explainers
(a)
Interpretation:
An element in Group
(b)
Interpretation:
An element in third period has to be named using the periodic table.
(c)
Interpretation:
An element that is present in Group
(d)
Interpretation:
An element that is present in Group
(e)
Interpretation:
A halogen preset in the fifth period has to be given using the periodic table.
(f)
Interpretation:
An alkaline-earth metal that is present in the third period has to be given using the periodic table.
(g)
Interpretation:
The noble gas element that is present in the fourth period has to be given using the periodic table.
(h)
Interpretation:
The nonmetal that is present in Group
(i)
Interpretation:
The metalloid that is present in the fourth period has to be named using the periodic table.
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Chemistry: The Molecular Science
- Fill in the blanks: (a) The symbol and atomic number of the heaviest alkaline earth metal are ______ and ______. (b) The symbol and atomic number of the lightest metalloid in Group 4A(14) are ______ and ______. (c) Group 1B(11) consists of the coinage metals. The symbol and atomic mass of the coinage metal whose atoms have the fewest electrons are ______ and ______. (d) The symbol and atomic mass of the halogen in Period 4 are ______ and ______.arrow_forwardv. Answer true or false. (a) Mendeleev discovered that, when elements are arranged in order of increasing atomic weight, certain sets of properties recur periodically. (b) Main-group elements are those in the columns 3A to 8A of the Periodic Table. (e) Nonmetals are found at the top of the Periodic Table, metalloids in the middle, and metals at the bottom. (d) Among the 116 known elements, there are approximately equal numbers of metals and nonmetals. (e) A horizontal row in the Periodic Table is called a group. () The Group 1A elements are called the "alkali metals." (g) The alkali metals react with water to give hydrogen gas and a metal hydroxide, MOH, where “M" is the metal. (h) The halogens are Group 7A elements. (1) The boiling points of noble gases (Group 8A elements) increase in going from top to bottom of the column.arrow_forwardHelium is the lightest noble gas and the second most abundant element (after hydrogen) in the universe. (a) The radius of a helium atom is 3.1x10-11 m; the radius of its nucleus is 2.5x10-15 m. What fraction of the spherical atomic volume is occupied by the nucleus (V of a sphere 5 4/ 3πr3)? (b) The mass of a helium-4 atom is 6.64648x10-24 g, and each of its two electrons has a mass of 9.10939x10-28 g. What fraction of this atom’s mass is contributed by its nucleus?arrow_forward
- 7. Isotopes. (a) Argon has three naturally occurring isotopes, 36Ar, 38Ar, and 40Ar. What is the mass number of each? How many protons, neutrons, and electrons are present in each? (b) Gallium has two naturally occurring isotopes, 6°Ga (isotopic mass = 68.9256 amu, abundance 60.11%) and 71Ga (isotopic mass = 70.9247 amu, abundance = 39.89%). Calculate the atomic mas of gallium.a %3D (c) Chlorine has two naturally occurring isotopes, 35CI (isotopic mass = 34.9689 amu) and 3"Cl (isotopic mass = 36.9659 amu). If chlorine has an atomic mass of 35.4527 amu, what is the percent abundance of each isotope?arrow_forward(a) In the certain hydrated salt MSO34H2O, the mass percentage of H2O is 44.71%.Identify the element M in the salt?(b) A certain element has two naturally occurring isotopes.The mass of one of the isotopes is 106.905 amu and its natural abundance is 51.60%.The mass of the second isotope is 108.883 amu.Calculate the average atomic massWrite the chemical symbols of the isotopes(c) An organic compound consists of carbon, hydrogen and sulfur only.The percentage of carbon by mass in this compound was found to be 30.27%.The complete combustion of 1.367 g this compound produces 1.765 g of sulfur dioxide(SO2) (i) Determine the empirical formula for this compound.(ii) If a sample of this compound having the mass 3.781 × 103 mg contains 9.528 × 10–3 molesof the compound, determine the molecular formulaarrow_forward(b) A certain element has two naturally occurring isotopes. The mass of one of the isotopes is 106.905 amu and its natural abundance is 51.60%. The mass of the second isotope is 108.883 amu. Calculate the average atomic mass Write the chemical symbols of the isotopesarrow_forward
- group and period. (a) Group 4A/14, Period 3; (b) Group 4A/14, Period 2; (c) Group 1B/11, Period 4; (d) Group 2A/2, Period 3. 42. I Write the atomic number of the element in each givenarrow_forward(d) the ion with 74 electrons, 116 neutrons, and a +3 chargearrow_forwardHydrogen sulfide is composed of two elements: hydrogen and sulfur. In an experiment, 6.500 g of hydrogen sulfide is fully decomposed into its elements. (a) If 0.384 g of hydrogen is obtained in this experiment, how many grams of sulfur must be obtained? (b) What fundamental law does this experiment demonstrate?arrow_forward
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