Zn will most likely get a 2+ (positive) charge!
yes, silver (along with cd, zn, sc, y, la &ac) is one of the few transition elements with a constant charge :)
One atom per molecule.
-2.37 V (apex) Chace
it says oxygen acts negativw so most likely hydrogen on the bottom acts positive
Compounds can be charged by different methods. But naturally most of the compounds are uncharged. So the overall charge of most compounds is neutral.
Zinc is Zn; bicarbonate, also known as hydrogen carbonate, is HCO3; after taking into account the +2 charge of the Zn and the -1 charge of HCO3 we get: Zn(HCO3)2.
+2 "God Speed and Party on" - Bas Rutten
I Think it would be Fe^2+
The oxidation number of Zn in the complex ion Zn(OH)4 2- is +2. This is because the overall charge of the complex ion is -2, and each hydroxide ion (OH-) has a -1 charge. Hence, the zinc (Zn) ion must have a +2 charge to balance the overall charge of the complex ion.
The charge of the Zn ion is typically 2+ or 2. This is because zinc typically loses two electrons to achieve a stable electron configuration.
Oxygen would most likely be reduced when combined with Zn(s) because zinc has a higher tendency to lose electrons and undergo oxidation, while oxygen has a higher tendency to gain electrons and undergo reduction.
Zn and K are more likely to form an ionic compound because zinc (Zn) readily loses two electrons to form a 2+ cation, while potassium (K) readily gains one electron to form a 1- anion, allowing for the formation of an ionic bond between the two elements.
The element with a density of 11.34 g/cm^3 is most likely zinc (Zn).
the charge of zinc has only one charge which is 2+.
ZnO is an ionic compound because it is made up of a metal (Zn) and a non-metal (O). Zinc (Zn) typically forms cations with a charge of +2, while oxygen (O) forms anions with a charge of -2, leading to the ionic bonding in ZnO.
Chlorine is most likely to form the chloride ion, which has a charge of -1.
The most likely ion charge for sodium (Na) is +1, as it typically loses one electron to achieve a stable electron configuration.