What element contains 34 protons?
What element contains 34 protons?
Selenium
What is the charge of an ion that has 34 protons and 36 electrons?
While the number nuclear protons as given is 34, and therefore we deal with the element selenium, there are 2 more electrons than protons, and therefore this species has an overall 2− charge. We represent this selenide ion as Se2−. Was this answer helpful?
What is the symbol of an ion with 33 protons 42 neutrons and 36 electrons?
#33 – Arsenic – As.
What is the charge of arsenic with 36 electrons?
Table of Common Element Charges
| Number | Element | Charge |
|---|---|---|
| 33 | arsenic | 3-, 3+, 5+ |
| 34 | selenium | 2-, 4+, 6+ |
| 35 | bromine | 1-, 1+, 5+ |
| 36 | krypton | 0 |
How many protons neutrons and electrons are present in the 59 28 Ni 2+ ion?
In nickel, 5928Ni, the 28 is the atomic number and 59 is the mass number. Therefore the number of protons = 28, the number of electrons is also 28, and the number of neutrons is 59-28=31.
How many protons are in co2+?
Write the complete chemical symbol for the ion with 84 protons, 125 neutrons, and 80 electrons….
| Ion | Number of Protons | Number of Electrons |
|---|---|---|
| Co+2 | 27 | 25 |
| Co+3 | 27 | 24 |
| Cl-1 | 17 | 18 |
| K+1 | 19 | 18 |
How many electrons are in the p3 ions?
The answer is 18. The atomic number of phosphorus is 15 and therefore the number electrons in a neutral phosphorus atom is only 15.
How many unpaired electrons are in P3?
We can see that the valence shell of P3- ion is 3s, 3p which is completely filled. A completely-filled orbital has no unpaired electrons. There are no unpaired electrons in the P3- ion.
How many unpaired electrons are in Na+?
Answer: The electronic configuration of Sodium(Na) is 1s2 2s2 2p6 3s1. In 1s, 2s and 2p orbitals have two electrons so they are paired but in 3s orbital only one electron is present so Sodium has one unpaired electron.
How many unpaired electrons are there in Fe3+?
5 unpaired electrons
What is the number of electrons in Fe3+?
23
What is the correct electron configuration for Fe 3+?
[Ar] 3d6 4s2
Why is FeI3 not stable?
Answer. I- is much larger in size, so has higher tendency to lose electron, and hence is a good reducing agent. I- reduces Fe3+ to Fe2+ and itself gets oxidised to I2, hence FeI3 is unstable. So, it being an oxidising agent oxidises Fe2+ to Fe3+, which favours formation of FeCl3 and makes it stable.
Why pbl4 does not exist?
Answer. PbI4 does not exist because the iodine reduces the lead to Pb(II) and the Pb oxidizes the iodine to iodine(I2). Since the iodine is not a strong reducuing agent to reduce Pb(II) to Pb, the compound Pbl2 is formed.