Solution:
For the easy removal of valence electron, the electron must be far from nucleus and having lower effective nuclear charge.
Reason: When electron is away from nucleus, then it experienced lesser force of attaction and hence easier will be its removal.
When effective nuclear charge is less, then the force of attaction of nucleus and valence electron is minimum, therefore removal becomes easier.
Therefore, option will be C.
Which description suggests an easier valence electron to be removed? Choose one electron close to nucleus,...
QUESTION 8 The effective nuclear charge felt by a valence electron in an atom is less than the atom's actual nuclear charge only when valence electrons are in the excited state. because core electrons are closer to the nucleus than the valence electrons. because valence electrons are more attracted to each other than the core electrons. o because core electrons partially shield the valence electrons from the charge of the nucleus.
_group 2? 2. Which element in group 1 has valence electrons closest to nucleus? 3. Valence electrons are closer or further from the nucleus going down a group? 4. Atomic radius increases or decrease moving down a group? 5. What is effective nuclear charge? (Definition)
stion 4 of 28 > Attempt The effective nuclear charge, Zef for a valence electron can be approximated using the core charge of the atom; that is, the total charge of the nucleus and the inner (nonvalence) electrons. Determine the core charge for an atom of Ar.
The energy states of atoms containing more than one electron arise from nucleus-electron and electron- electron interactions. Which of the following statements correctly describes these effects? O Larger nuclear charge lowers energy; more electrons in an orbital lowers energy. O Larger nuclear charge lowers energy; more electrons in an orbital increases energy. O Smaller nuclear charge lowers energy; more electrons in an orbital lowers energy, O Smaller nuclear charge lowers energy; more electrons in an orbital increases energy. O None...
Which element in Group I has the lowest effective nuclear charge, Zeff, for a valence electron? Answer with correct elemental symbol
A. If an element with the valence configuration 4s2loses 2 electron(s), these electron(s) would be removed from the _______spdfs + ps + dp + d subshell(s). B. An element with the valence electron configuration 2s22p4would form a monatomic ion with a charge of ________ . In order to form this ion, the element will _____lose/gain ___12345678 electron(s) from/into the _______spdfs + ps + dp + d subshell(s).
Rank the effective nuclear charge Z* experienced by a valence electron in each of these atoms: atom z* experienced by a valence electron. An atom of phosphorus. (pick one) An atom of argon. (pick one) An atom of sulfur. (pick one), An atom of magnesium. (pick one) x | ?
A.If an element with the valence configuration 4s23d8 loses 2 electron(s), these electron(s) would be removed from the (answer) subshell(s). B. An element with the valence electron configuration 2s22p5 would form a monatomic ion with a charge of (answer). In order to form this ion, the element will (answer) (lose/gain) electron(s) from/into the(answer) subshell(s).
Rank the effective nuclear charge Z experienced by a valence electron in each of these atoms: atom z* experienced by a valence electron. An atom of sodium. (pick one) 1 (highest) An atom of aluminum. 4 (lowest) An atom of sulfur. (pick one) An atom of phosphorus. (pick one)
7) Choose the statement that is TRUE. A) f electrons completely shield valence electrons from nuclear charge. B) Valence electrons partially shield one another from nuclear charge. C) Valence electrons experience the most shielding in an atom. D) According to Slater's Rules, shielding ranges from 0.3 to 1. E) Core electrons have the strongest attraction to the nucleus. F) All of the above are correct. ID: exal num Dept 8) Place the following in order from lowest to hightest metallic...