2014年4月18日 · Turns out the silver-107 and silver-109 are almost equally abundant, making the average atomic mass nearly 108. Once you know that the two isotopes have masses of nearly 107 and 109, you can determine which one is more …

2023年9月18日 · Complete the following table, showing the number of protons, neutrons, and electrons for the two most common isotopes of mercury (200^Hg and 202^Hg) in both the elemental and ion forms. In this compound, mercury forms an ion with a charge of +2, and sulfur forms an ion with a charge of −2.

Summer R. asked • 10/08/18 An element has two common isotopes. 98.89% of its atoms have an atomic mass of 12.09 amu, whereas the other 1.11% have an atomic mass of 13.10 amu.

2015年7月20日 · Let's get a tally of the number of electrons, neutrons, and protons for these three isotopes: 20 Ne 10 protons, given by atomic number (look at your periodic table)

Layla J. asked • 02/01/21 Argon has three common isotopes, with the masses and isotopic abundances shown below

2019年9月11日 · Copper (Cu) has two common isotopes. One isotope has 34 neutrons and 29 protons, and it accounts for 69.15% of all copper. The other isotope has 36 neutrons and 29 protons and it accounts for 30.85% of all copper. Using the isotopic composition provided, calculate the average atomic mass of copper. Round your answer to the tenths place.

2017年6月2日 · This will tell you that there are slightly more bromine-79 than bromine-81 among the bromine isotopes that have been found so far. The best choice is c. If you want to find the % of each bromine isotope, just solve the following equation for x.

2016年7月9日 · Oxygen is composed of three isotopes: oxygen-16, oxygen-17 and oxygen-18 and has an average atomic mass of 15.9980 amu. Oxygen-17 has a mass of 16.992 amu and makes up 0.035% of oxygen. Oxygen-16 has a mass of 15.982 amu and Oxygen-18 has a mass of 17.984 amu. What is the percent abundance of Oxygen-18?

some common isotopes of carbon are carbon-13 and carbon-14, which can be interpreted as follows: carbon-13 would have 6 protons and 6 electrons (as usual) but this isotope would have 7 neutrons, as 13 – 6 = 7. Carbon-14 would have 6 protons and 6 electrons, as usual, but this isotope would have 8 neutrons, as 14 – 6 = 8.

Magnesium consists of three naturally occurring isotopes. The percent abundance of these isotopes is as follows: 24Mg (78.70%), 25Mg (10.13%), and 26Mg (11.7%). The average atomic mass of the three isotopes is 24.3050 amu. If the atomic mass of 25Mg is 24.98584 amu, and 26Mg is 25.98259 amu, calculate the actual atomic mass of 24Mg.