3.8 Extensions of Electron Configurations (Chemistry)

What is the symbol for the following ion electronic structure: [Ne]3s^2 3p^6 with an atomic number of 16?

S^{2-} Atomic number 16 corresponds to S but there are 2 more electrons than S usually has so we know that S had to gain (−2).

Which of the following elements are part of the "p block" on the periodic table? (Select all that apply)

Select all that apply: [-]Boron []Platinum [-]Silicon []Calcium The "p block" elements are on the right side of the periodic table. The p orbital holds 6 electrons which makes sense since there are 6 groups in the p block.

What defines how elements react?

[]the loss of valence electrons []the gaining of valence electrons []the sharing of valence electrons [-]all of the above

What is the electron configuration for O2−?

1s^2 2s^2 2p^6

Which element has an electron configuration ending in 4p^5

Br Bromine is in period 4 and is the fifth element in the corresponding p block, so its electron configuration will end in 4p^5

Which of the following is a rule indicated by the Aufbau principle?

Electrons are placed in the lowest energy subshell that is not fully occupied. The Aufbau principle indicates that electrons are placed in the lowest energy subshell that is not already fully occupied. This order is illustrated by the image below. Different subshells have different capacities and each subshell will be filled before moving on to the next subshell. The s subshells hold 2 electrons. The p subshells hold 6 electrons. The d subshells hold 10electrons. The f subshells hold 14 electrons.

Elements in one group have _______ number of valence electrons.

Elements in one group have the same number of valence electrons.

What is the ground state configuration of calcium? (Ca)

[Ar] 4s^2

What is the abbreviated electron configuration of cesium?

[Xe]6s^1 The noble gas from the row above is xenon, so we will need xenon core plus the 6s valence electron.

Valence electrons:

[]are available to do chemistry and participate in covalent bonding []have the highest energy []are lost first [-]all of the above

Which of the following statements about nonmetals is true?

[]ligand field strength []oxidation state of the central atom []geometry of the complex [-]all of the above

For the purposes of determining electron configuration of ions, when electrons are added to a neutral atom, they will inhabit orbitals according to:

[]the Pauli exclusion principle []the Aufbau principle []Hund's rule [-]all of the above

Which block does selenium belong to?

p block

How many electrons can an f subshell hold?

14 The value of ml determines the number of orbitals in a subshell. Each orbital can hold a maximum of 2 electrons so for subshell f (ml values of −3,−2,−1,0,+1,+2,+3) there can be 14 electrons.

Which element has the electron configuration 1s^2 2s^2 2p^6 3s^1?

Na

Which element has the core electrons 1s22s22p6?

Na Sodium has one valence electron in the 3s orbital, so all the electrons that have n=2 or less can be considered core electrons.

Which core electrons are implied by the symbol [Ne]?

1s^2 2s^2 2p^6 Neon has the electron configuration 1s^2 2s^2 2p^6, so these are the core electrons that are implied when an element is listed as having a neon core.

What are the core electrons of strontium?

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 Strontium's full electron configuration is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6. To find its core electrons, we must separate the valence electrons (in this case, 5s2) from all of the complete principal energy level shells (the configuration of the closest noble gas). Thus we isolate the electron configuration of krypton, 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 from the full electron configuration of Sr. These are its core electrons, which are virtually unreactive as they constitute full octets.

What is the electron configuration of tellurium (Te)?

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10 }5p^4 Tellurium is in the fifth period and a member of group 16. The atomic number of tellurium is 52 so there must be 52electrons in the electron configuration for a neutral tellurium atom. Therefore, the electron configuration for tellurium is 1s22s22p63s23p64s23d104p65s24d105p4 [Kr]5s^2 4d^10 5p^4

The electron configuration for sodium is 1s^2 2s^2 2p^6 3s^1. Which subshell is said to contain the valence electron(s) for sodium?

3s For main group elements, the shell with the largest value of n is called the valence shell. In this case, the subshell with the largest value of n is the 3s subshell (n=3), and so the single valence electron in sodium is held in the 3s subshell.

What is the configuration for the valence electrons in chlorine?

3s^23p^5 Chlorine's full electron configuration is: 1s^2 2s^2 2p^6 3s^2 3p^5. The valence electrons are those in the highest energy level, in this case the 3s^2 3p^5.

The orbitals that are next highest in energy after the 5s orbitals are the:

4d

What is the electron configuration of Ge?

Germanium contains 32 protons and electrons and using the electron configuration order (1s,2s,2p,3s,3p,4s,3d,4p,5s,4d,5p,6s,4f,5d,6p,7s,5f,6d,7p,8s), can fill up to 32 which gives us the answer. Therefore the electron configuration for germanium is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^2

Which core electrons are implied by the symbol [He]?

Helium has an electron configuration of 1s2, so these are the core electrons that are implied when an element is listed as having a helium core.

The electrons occupying the innermost shell orbitals are known as:

core electrons The electrons occupying the innermost shell orbitals are known as core electrons.

Which block does uranium belong to?

f block

Which of the following has the last electron added into the f orbital?

inner transition elements Inner transition elements are metallic elements in which the last electron added occupies an f orbital. The valence shells of the inner transition elements consist of the (n - 2)f, the (n - 1)d, and the ns subshells.

Each row on the periodic table corresponds to which quantum number for s and p orbitals?

principal quantum number The period or row number corresponds to the n value which is the principle quantum number for the orbital subshells. Therefore, elements in row 1 fill the 1 s orbital. Elements in row 2 begin to fill the 2 s and 2 p orbitals, and so on. Notice though, that when the d and f subshells begin these start at n−1 and n−2, respectively.