1) the element Q has the electronic configuration 1S2, 2S2, 2p6, 3s2, 3p6, 4s2 3d10, 4p1. Write the atomic #. Q exist as 69Q and 71Q. What is the significance of the 2 #'s. What does it mean.
B) find the atomic mass if 69Q is 60% anf 71Q is 40%
A) The atomic number (Z) represents the number of protons in the nucleus of an atom, which identifies the element. In this case, you are given the electronic configuration of element Q as 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p1. By counting the electrons, you can determine the atomic number.
The electronic configuration consists of energy levels and sublevels, where the number before the letter represents the energy level, and the letter represents the sublevel. Each sublevel can hold a specific number of electrons:
- 1s sublevel can hold up to 2 electrons.
- 2s sublevel can hold up to 2 electrons.
- 2p sublevel can hold up to 6 electrons.
- 3s sublevel can hold up to 2 electrons.
- 3p sublevel can hold up to 6 electrons.
- 4s sublevel can hold up to 2 electrons.
- 3d sublevel can hold up to 10 electrons.
- 4p sublevel can hold up to 6 electrons.
Adding up the total number of electrons, we find:
(2 + 2 + 6 + 2 + 6 + 2 + 10 + 1) = 31
Therefore, the atomic number of element Q is 31.
As for the significance of the two numbers (69Q and 71Q), they typically represent different isotopes of the same element. Isotopes are atoms of the same element but with different numbers of neutrons. The atomic number (Z) remains the same, but the mass number (A) changes. In this case, the different numbers indicate that there are two isotopes of element Q: one with a mass number of 69 and another with a mass number of 71.
B) To find the atomic mass, you need to consider the percentage abundance of each isotope. In this case, 69Q is 60% abundant and 71Q is 40% abundant.
To calculate the atomic mass, you use the formula:
Atomic mass = (mass of isotope 1 × % abundance of isotope 1) + (mass of isotope 2 × % abundance of isotope 2)
Substituting the values given:
Atomic mass = (69 × 0.60) + (71 × 0.40)
= 41.4 + 28.4
= 69.8
Therefore, the atomic mass of element Q is approximately 69.8.
To find the atomic number of an element, you need to look at its electronic configuration. In this case, the element Q has the following electronic configuration: 1S2, 2S2, 2p6, 3s2, 3p6, 4s2 3d10, 4p1.
To determine the atomic number, we need to count the total number of electrons in the configuration. Counting the electrons, we get:
1S2 (2 electrons)
2S2 (2 electrons)
2p6 (6 electrons)
3s2 (2 electrons)
3p6 (6 electrons)
4s2 3d10 (12 electrons)
4p1 (1 electron)
Adding up all the electrons, we get:
2 + 2 + 6 + 2 + 6 + 12 + 1 = 31
Therefore, the atomic number of element Q is 31.
Regarding the two different symbols, 69Q and 71Q, the numbers 69 and 71 represent the atomic mass of the isotopes of element Q. Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons. The atomic mass of an element is the weighted average of the masses of its isotopes.
In this case, if 69Q and 71Q are the isotopes of element Q, and 69Q is present at 60% and 71Q is present at 40%, you can calculate the atomic mass as follows:
Atomic mass = (mass of 69Q) * (fractional abundance of 69Q) + (mass of 71Q) * (fractional abundance of 71Q)
Assuming the masses of 69Q and 71Q are 69 amu and 71 amu respectively, we can calculate the atomic mass as:
Atomic mass = (69 amu) * (0.60) + (71 amu) * (0.40)
= 41.4 amu + 28.4 amu
= 69.8 amu
Therefore, the atomic mass of element Q, considering the given abundances of 69Q and 71Q, would be 69.8 amu.
A. Count the electrons. #e = # protons = atomic number.
The two numbers are the mass numbers of the two isotopes of element 31.
B. You need the atomic mass for the isotope of 69 and 71. Assuming they are 69 and 71 (that isn't quite correct), that will be
(0.60*69) + (0.40*71) = ?