For the following questions, consider the element whose full ground-state electron configuration is 1s°2s²2p°3s?3p°4s?3dlº4p°5s²4d!©5p%. • a. Write the name of this element? b. How many of its electrons are valence electrons? c. Write the full set of allowed quantum numbers for the 4d orbital? d. Determine the total number of nodes in the 5p orbital. How many are angular? How many are radial?

An electron has the following set of quantum numbers: 3, 2, -1, -12. L L L What is the energy level for this electron? What type of orbital is represented by these quantum numbers? Which of the following atoms could have an electron in the ground state with these quantum numbers?

Which of the following subshells has room for 10 electrons? 5s 4p 2p 3d 3p

For each of the following sets of quantum numbers, determine how many electrons in a single atom could have that specific set of numbers. n = 2 Number: n = 4, l=1 Number: n = 5,l=1, m₁ = 0 Number: electrons electrons electrons

In one atom, what is the maximum number of electrons that could have the quantum number of n = 3? electrons 1 3 4 6. C 7 8 9. +/- х 100 +

Hi! Wouldn't there only be five answers (and not 10) for the quantum numbers since the electrons in the d-orbitals are unpaired?

Fix any errors in these proposed electron configurations. number of electrons in atom 16 5 26 proposed electron configuration 6 15 1p 2s 2p 15²25²35²¹ 15 25 2p 3s 3p 3d

please solve question 1 and  2, thanks alot sir

The Pauli Exclusion Principle tells us that no two electrons in an atom can have the same four quantum numbers. In progress For an electron in the 3s orbital shown above, enter a possible value for each quantum number. n = 1 = = Give ONE example. Give ONE example. Though a given electron only has one value for possible mi, there are my values for electrons in 3s orbitals. m₁ = ms = Submit Answer Retry Entire Group 9 more group attempts remaining