0
no. it's d sublevel is full and that is the reason why it is not coloured like other transition metals that have a partially filled d-sublevel
Wiki User
∙ 13y ago
Add your answer:
Earn +20 pts
What is the least reactive element in the group 2 of the periodic table of elements?
The Zinc Family also known as group IIB is the second least reactive I believe. The least reactive family is the one with a full p sublevel, the noble gases, the next least reactive would be the family with a full d sublevel. Since group IIB has a full d sublevel, it must be the next least reactive family.
What is Zn3P2?
Zinc Phosphide ;D
Is zink organic?
Zinc and compounds of zinc are inorganic due to absence of carbon.
Is silicon a transition element?
No, silicon is not a transition element. It is a metalloid located in Group 14 of the periodic table. Transition elements are defined as elements that have partially filled d sublevels in one or more of their oxidation states.
What is another name for zinc?
Another name for Zinc is "Zink" if I'm not mistaken. :D Against part: zink is the miss spelling of zinc so that is not the answer
Which subshells of transition metals are partially filled?
D sublevel
Which of the d-block elements are not regarded as transition metals?
Scandium and zinc (and probably those below them in their groups, but I'm uncertain of that) are not considered to be transition metals, as they do not form ions with partially filled d-subshells.
Why is copper a transition metal as it have completely filled d sub-shell?
Copper is a transition metal because it can easily lose its valence electron from the s orbital to form a +2 oxidation state. This electron loss creates a partially filled d orbital, allowing copper to exhibit typical transition metal properties such as variable oxidation states and complex formation.
When do D orbitals start gettin filled?
D orbitals start to get filled after the 3p orbitals in the periodic table. They are typically filled after filling the 4s orbital, as the 3d orbitals are the next to be filled in the transition metal series.
Which sublevels of the third energy level are filled in the element krypton?
In the element krypton, the third energy level has 3 sublevels: s, p, and d. The s and p sublevels are filled first before the d sublevel. This means that in krypton, the 4s and 4p sublevels are filled, while the 4d sublevel remains empty.
Elements in which the d-sublevel is being filled have the properties of?
Elements in which the d-sublevel is being filled have properties such as variable oxidation states, colored compounds, and the ability to form complex ions due to the arrangement of electrons in the d orbitals. These elements typically exhibit metallic behavior and can form transition metal compounds with unique chemical and physical properties.
The first transition series represents the filling of the orbital?
The first transition series includes the filling of the 3d sublevel orbitals in transition metal elements from Scandium (Sc) to Zinc (Zn). These elements gradually fill the 3d orbital with electrons as they progress across the period, leading to the formation of various oxidation states and colorful compounds due to the presence of partially filled d orbitals.
Are transition metal good catalysts?
because of partially filled d orbitol
Where does the final electron in inner transition metals enter?
It enters the f sublevel.
How many d orbital can there be in an energy level?
The d sublevel contains 5 orbitals
Why electronic configuration of copper is 1s2 2s2 2p6 3s2 3p6 4s1 3d10 and why not 1s2 2s 2p6 3s2 3p6 4s2 3d9?
The electronic configuration of copper is 1s2 2s2 2p6 3s2 3p6 4s1 3d10 because it is more stable to have a completely filled d-orbital (3d10) and a half-filled s orbital (4s1). This arrangement follows Hund's rule which states that electrons fill up orbitals singly before pairing up. Therefore, the 4s orbital loses an electron to completely fill the 3d orbital.
Why zinc produces colourless compounds?
Zinc typically forms colorless compounds because it lacks partially filled d or f orbitals that are responsible for absorbing visible light and producing color. This leads to zinc compounds having no electronic transitions in the visible light range, resulting in their colorless appearance.
