40
Ca2+
20
79
Br-
35
58
Ni2+
28
For the three ions written above give the correct number of each of the following:
a) the maximum number of electrons in the first shell
b)the unpaired electrons in an oxygen atom
c)the full orbitals in a chlorine atom
d)the number of types of f-orbitals
Please help and explain clearly and fully im really confused
You need an inperson tutor. Being "really confused" and not being able to ask specific questions is not conducive to online tutoring.
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a) To determine the maximum number of electrons in the first shell, you need to know the principal quantum number (n) for the shell. The principal quantum number refers to the energy level or shell number in an atom.
For the first shell (n=1), the formula to calculate the maximum number of electrons it can hold is given by 2n^2. Plugging in n=1 into the formula, we get:
Maximum number of electrons in the first shell = 2(1)^2 = 2(1) = 2
Therefore, the maximum number of electrons in the first shell is 2.
b) To find the number of unpaired electrons in an oxygen atom, you need to determine its electron configuration. The electron configuration of oxygen is 1s^2 2s^2 2p^4.
The electron configuration shows the distribution of electrons in different atomic orbitals. In the case of oxygen, the electrons fill the 1s, 2s, and 2p orbitals.
In the 2p orbital, there are 3 orbitals available (2px, 2py, and 2pz), with each orbital capable of holding a maximum of 2 electrons.
Since oxygen has 4 electrons in the 2p orbital, we know that there must be one unpaired electron. Therefore, the number of unpaired electrons in an oxygen atom is 1.
c) To determine the number of full orbitals in a chlorine atom, we need to consider its electron configuration. The electron configuration of chlorine is 1s^2 2s^2 2p^6 3s^2 3p^5.
In chlorine's electron configuration, all the orbitals in the first and second energy levels (1s, 2s, and 2p) are filled. This accounts for a total of 8 electrons.
Since there are no electrons in the 3s orbital yet, it is not considered a full orbital. However, in the 3p orbital, there are 5 electrons. Since each of the 3p orbitals can hold a maximum of 2 electrons, we can say that there is one full orbital in the 3p sublevel.
Therefore, a chlorine atom has one full orbital in the 3p sublevel.
d) The number of types of f-orbitals is determined by the value of the azimuthal quantum number (l) for the f-sublevel. The azimuthal quantum number represents the shape of the orbital.
For the f-sublevel, the possible values of l range from -3 to +3. Therefore, there are 7 possible values of l for the f-orbitals: -3, -2, -1, 0, 1, 2, 3.
Since each value of l corresponds to a different orbital shape within the f-sublevel, we can say that there are 7 types (or shapes) of f-orbitals.
Therefore, there are 7 types of f-orbitals.