Write the atomic symbol (X) for each of the isotopes described below. a. number of protons = 27. number of neutrons = 31 b. the isotope of boron with mass number 10 c. Z - 12, A= 23

Gallium consists of two isotopes, gallium-69 and gallium-71. Gallium-69 has a mass of 68.926 u and a fractional abundance of 0.601. Determine the mass of the gallium-71 isotope.

D Suppose that fictional element X has an average atomic mass of 74.029 u. Element X has two isotopes. One isotope has a mass of 72.021 u and a percent abundance of 24.43%. Calculate the mass of the second isotope. mass of second isotope: x10 TOOLS u

An element has two naturally occurring isotopes. Isotope 1 has a mass of 190.9606 amu and a relative abundance of 37.3%, and isotope 2 has a mass of 192.9629 amu. - Find the atomic mass of this element.

a. Using the average atomic mass of carbon, calculate the mass (in amu) of 227 carbon atoms. amu b. Using the average atomic mass of potassium, calculate the mass (in amu) of 4.80 × 106 potassium atoms. amu c. Using the average atomic mass of lithium, calculate the mass (in amu) of 8.80 × 10²3 of lithium atoms. amu d. Using the average atomic mass of magnesium, calculate the mass (in amu) of 5 magnesium atoms. amu e. Using the average atomic mass of iodine, calculate the mass (in amu) of 8.300 × 10²³ iodine atoms. amu

A) Calculate the mass of a gold-197 atom using the information from question 9 and the masses of the subatomic particles listed below. B) Calculate the volume of the gold atom in cm3. C) Calculate the density of the gold atom in g/ cm3. Report the density of the gold atom to the correct number of significant figures. All other calculations should not be rounded or carry at least 2 extra significant figures. Mass of neutron 1.675 x 10-24 g Mass of proton 1.673 x 10-24 g Mass of electron 9.109 x 10-28 g Atomic radius of gold 1.66 x 10-10 m Volume of a sphere (4/3)(π)(r3)

Find the average atomic mass of this isotope of an unknown element. mass 1 220.9038. abundance 100% mass 2 222.9041 abundance 74.8%

Sulfur is a bright yellow solid at room temperature. It is one of the components in gunpowder, matches, and fireworks. It is added to rubber to make it tougher (vulcanization) and to topical ointments for the treatment of skin disorders. a. What is the molecular formula? b. How many electrons and protons are there in an atom of sulfur? c. Two atoms of sulfur combine with two atoms of chlorine. Is this compound a molecule? What is its name and formula? d. How many neutrons are there in the isotope S-36? e. The naturally occurring isotopes of sulfur, their atomic masses, and abundances are: S-32 :31.97207 amu – 94.93% S-33 : 32.97146 amu – 0.76 % S- 34: 33.96786 amu – 4.29 % S- 36 :35.96708 amu – 0.02 % What is the average atomic mass for sulfur? Show the detailed solution. f. How many atoms are there in 12.55 grams of elemental sulfur (S) ? g. What is the mass of a billion atoms of sulfur? h. Sulfur can combine with oxygen in many different ways. Give five examples of that compound and…

Q.3 A neutral atom has a mass number of 80 and has 45 neutrons. Write its complete symbol. Q.4 An atom has two more protons and two more electrons than the atom in question 3. What is its complete symbol?

20. How many protons, electrons, and neutrons are in each isotope? electrons, and neutrons. protons; B) 2Tm protons; protons: clectrons, and klectrons, and ncutrons. neutrons.