He 2A 3A 4A SA 6A 7A Li Be B C NOF Ne Na Mg 38 Al Si S C Ar 48 58 68 78 18 28 K Ca Sc Ti v Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Give the spectroscopic notation (also called spdf notation) electron configuration of P. Enter the subshells in the order in which they are filled. For example, for oxygen, the answer would be: 1s 25 2p*.

For the following atoms, fill out the electron configuration and write out the arrow notation:   Electron  Configuration 1s 2s 2p 3s 3p 4s 3d Mg                 Ge                 Si                 Ca^2+                 Cl^-

The Pauli Exclusion Principle tells us that no two electrons in an atom can have the same four quantum numbers. For an electron in the 3p 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 3p orbitals. m₁ = mg = Submit Answer Retry Entire Group 9 more group attempts remaining

Some patterns of electron configuration are listed below. In each case, [G] stands for a noble-gas core and n, m, or o stand for integer numbers like 1, 2, 3 and so on. Note: assume G is lighter than Rn. Think about the chemical elements made of atoms with an electron configuration that matches each pattern. In what block or blocks of the Periodic Table would these elements lie? Would they be metals, nonmetals, metalloids, some of each? Use your answers to these questions to complete the table. electron configuration of atoms 6 [G]ns²np [G]ns¹ 2 [G]ns²mf³ 3 blocks 00 P S 00 P 00 S location of elements (check all that apply) S C р р f р f metals or nonmetals? 000 000 000 metals nonmetals metalloids metals nonmetals metalloids metals nonmetals metalloids

D. Give the quantum numbers for the last electron of each element given in Part II following the table below. Element 1 subshell N - 7 1s22s22p3 70 Ga,17⁰ Ar 1840 Sb,1122 112 AU79197 n main energy level 2 s=0 p=1 d=2 f=3 1 m₁ orbital -1 to 0 to +1 -1, 0, +1 +1 m₂ magnetic spin (+1/2, -1/2) +1/2

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 +

Some patterns of electron configuration are listed below. In each case, [G] stands for a noble-gas core and n, m, or o stand for integer numbers like 1, 2, 3 and so on. Note: assume G is lighter than Rn. Think about the chemical elements made of atoms with an electron configuration that matches each pattern. In what block or blocks of the Periodic Table would these elements lie? Would they be metals, nonmetals, metalloids, some of each? Use your answers to these questions to complete the table. electron configuration of atoms 2 [G]ns²mfs 5 3 [G]ns² md¹np³ [G]ns²md¹np 6 blocks 00 00 S e S S location of elements (check all that apply) a U 0 00 р f р f р f metals or nonmetals? 00 000 0 0 0 X metals nonmetals metalloids metals nonmetals metalloids metals nonmetals metalloids Ś

Fix any errors in these proposed electron configurations. number of electrons in atom 14 8 23 proposed electron configuration S 15 25² 2p 35² 2 6 1s 1p 2 6 2 15 25² 2p 35² 3p 3d³ T ATTENTREMANSTENSTRASTICA MOCOTESTANT sz (STADIO Statestatas Russiese casco X

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