nooo idea how to do these:

Identify the oxidation numbers for each element in the following equations. Then determine whether each equation describes a redox reaction. Justify your answer in terms of electron transfer. Describe the oxidation and reduction that occurs.

a. Ca + 2HCl -- CaCl2 + H2

b. 2KOH + K2Cr2O7 -- 2K2CrO4 + H2O

Question

nooo idea how to do these:

Identify the oxidation numbers for each element in the following equations. Then determine whether each equation describes a redox reaction. Justify your answer in terms of electron transfer. Describe the oxidation and reduction that occurs.

a. Ca + 2HCl --> CaCl2 + H2

b. 2KOH + K2Cr2O7 --> 2K2CrO4 + H2O

anonymous · Answer

@JoannaBlackwelder ?

abmon98 · Answer

The oxidation state of an uncombined element is zero.
The sum of the oxidation states of all the atoms or ions in a neutral compound is zero.
Group 2 metals always has an oxidation state of +2
Group 1 metals	always has an oxidation state of +1
Hydrogen	usually +1	except in metal hydrides where it is -1
a) Ca:0 H:+1 Cl:-1 on the reactant side on the product side Ca:+2 Cl2:-2 H2:0

anonymous · Answer

@Abmon98 how do i do the rest of this though?