Because 4s is a lower energy level and 3d is higher. In fact, s levels should, strictly, be written first before d levels when writing electron configurations.
Sc is a 3d element. It has 21 protons and 21 electrons.
In actuality Mn has SEVEN valence electrons, not really 2 as might be predicted. The reason for this is that Mn is [Ar]3d5 4s2, and as a transition element, not only are the 4s electrons available for bonding, but so are those in the d orbital. So, the 5 electrons in 3d and the 2 electrons in 4s are all considered as valence electrons.
Chromium is a 3d element. and cobolt also a 3d element.
That is correct. Titanium has 22 electrons, and its highest full orbital is 4s and the 3d is partially filled with 2 electrons. So Titanium is 1s22s22p63s23p64s23d2
because its energy level is lower
The 3d subshell is completely filled in Arsenic. Therefore it has 10 electrons.
Niobium (Nb) Because three 4d electrons = 3d^3
Sc is a 3d element. It has 21 protons and 21 electrons.
1s22s22p63s23p64s23d5
Lithium atoms have three electrons.
vanadium (V)
The 4s orbital falls in a slightly lower energy level than the 3d orbital when it is empty so it will fill with electrons first, but when it is full of electrons it rises to be above the 3d one so that it will lose electrons first as well.
On the periodic chart, the element with 5 electrons in its 3d orbital can be quickly identified. Elements with partially filled d-orbitals are located in the middle section, the "transitional metals." 3d is the first d-orbital, so we look in the first row of the middle section. This section fills the orbital by one more electron per element, so the one with 5 electrons is the fifth from the left.... Manganese! Atomic number 25.
The 3d sub-level has 5 orbitals, and therefore space for a total of 10 electrons. Excluding certain hyper-valent bonding scenarios, the first element with electrons to occupy the 3d sub-level is scandium (Sc).
Zinc has ten 3d electrons.
3d
3d10 Ten electrons is the maximum number of electron in 3d.