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Problem 105c
How many protons and neutrons are in the nucleus of the following atoms? (c)
Problem 105d
How many protons and neutrons are in the nucleus of the following atoms? (d)
- Identify the following elements: (a)
Problem 106
- Which of the following isotope symbols can't be correct? (a) (b) (c) (d)
Problem 108
Problem 109
The molar mass of HCl is 36.5 g/mol, and the average mass per HCl molecule is 36.5 u. Use the fact that 1 u = 1.6605 * 102 24g to calculate Avogadro's number.
- Fluorine occurs naturally as a single isotope. How many protons, neutrons, and electrons are present in deuterium fluoride (2HF)? (Deuterium is 2H.)
Problem 110
- Hydrogen has three isotopes (1H, 2H, and 3H), and chlorine has two isotopes (35Cl and 37Cl). How many isotopic kinds of HCl are there? Write the formula for each, and state how many protons, neutrons, and electrons each contains.
Problem 111
- The unified atomic mass unit (u) 1/12 the mass of a neutral atom of: (a) 1^H (b) 12^C (c) 14^C (d) 16^O
Problem 112
Problem 113a
(a) The unified atomic mass unit (u) is used to represent the extremely small mass of atoms. How many grams are equivalent to 1 u?
Problem 113b
(b) The mole is a unit used to represent a very large number of atoms. How many atoms are equivalent to 1 mol of atoms?
- Match the descriptions (a)–(e) with the following terms: atomic weight, atomic mass, mass number, atomic number, molar mass. (a) The mass of a specific atom such as one atom of 13C (b) The quantity determined by the number of protons in an element. (c) The number of grams in 1 mol of an element (d) The number of protons and neutrons in an element (e) The weighted average of the isotopic masses of an element's naturally occurring isotopes
Problem 114
- Label the following statements as true or false. (a) The atomic weight and the atomic number of an element have the same numerical value. (b) The molar mass in grams for an element and the atomic weight have the same numerical value.
Problem 115
- Copper has two naturally occurring isotopes, including 65Cu. Look at the periodic table and tell whether the second isotope is 63Cu or 66Cu.
Problem 116
- A copper wire having a mass of 2.196 g was allowed to react with an excess of sulfur. The excess sulfur was then burned, yielding SO2 gas. The mass of the copper sulfide produced was 2.748 g. (c) Calculate the number of copper ions per cubic centimeter if the density of the copper sulfide is 5.6 g/cm3.
Problem 117
- Naturally occurring boron consists of two isotopes: 10^B (19.9%) with an isotopic mass of 10.0129 and 11^B (80.1%) with an isotopic mass of 11.009 31. What is the atomic weight of boron? Check your answer by looking at a periodic table.
Problem 118
Problem 119
Naturally occurring silver consists of two isotopes: 107^Ag (51.84%) with an isotopic mass of 106.9051 and 109^Ag (48.16%) with an isotopic mass of 108.9048. What is the atomic weight of silver? Check your answer in a periodic table.
Problem 120
Magnesium has three naturally occurring isotopes: 24Mg (23.985) with 78.99% abundance, 25Mg (24.986) with 10.00% abundance, and a third with 11.01% abundance. Look up the atomic weight of magnesium, and then calculate the mass of the third isotope.
- A sample of naturally occurring silicon consists of 28^Si (27.9769), 29^Si (28.9765), and 30^Si (29.9738). If the atomic weight of silicon is 28.0855 and the natural abundance of 29^Si is 4.68%, what are the natural abundances of 28^Si and 30^Si?
Problem 121
- Copper metal has two naturally occurring isotopes: copper-63 (69.15%; isotopic mass = 62.93) and copper-65 (30.85%; isotopic mass 64.93). Calculate the atomic weight of copper, and check your answer in the periodic table.
Problem 122
- Germanium has five naturally occurring isotopes: 70^Ge, 20.5%, 69.924; 72^Ge, 27.4%, 71.922; 73^Ge, 7.8%, 72.923; 74^Ge, 36.5%, 73.921; and 76^Ge, 7.8%, 75.921. What is the atomic weight of germanium?
Problem 123
- What is the mass in grams of each of the following samples? (a) 1.505 mol of Ti (b) 0.337 mol of Na (c) 2.583 mol of U
Problem 124
- How many moles are in each of the following samples? (a) 11.51 g of Ti (b) 29.127 g of Na (c) 1.477 kg of U
Problem 125
- If the atomic weight of an element is x, what is the mass in grams of 6.02 x 10^23 atoms of the element? How does your answer compare numerically with the atomic weight of element x?
Problem 126
- If the atomic weight of an element is x, what is the mass in grams of 3.17 * 1020 atoms of the element?
Problem 127
- If 6.02 * 1023 atoms of element Y have a mass of 83.80 g, what is the identity of Y?
Problem 128
- If 4.61 * 10^21 atoms of element Z have a mass of 0.815 g, what is the identity of Z?
Problem 129
Problem 130a
Refer to Figure 2.10 showing a schematic illustration of a mass spectrometer. (a) What is the purpose of bombarding the gaseous atoms with an electron beam?
Problem 130b
Refer to Figure 2.10 showing a schematic illustration of a mass spectrometer. (b) Compare two ions with a +1 charge traveling through the curved, evacuated tube in the mass spectrometer. Will a heavier ion or lighter ion be deflected to a greater degree by the magnetic field?
- Use the data from the mass spectrum of a sample of an element to calculate the element's atomic weight. Identify the element.
Problem 132
- Use the data from the mass spectrum of a sample of an element to calculate the element's atomic weight. Identify the element.
Problem 133