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Is this a reduction oxidation reaction If so, wh.pdf

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Is this a reduction oxidation reaction? If so, what you use is the periodic table. Hydrogen will always have a +1 charge associated with it and Br and F are both halogens which have a -1 charge associated with them. For your reaction, Hydrogen is staying constant at +1 while Br is going from -1 to 0 and F is going from 0 to -1. When atoms are bound to other atoms, they display a charge. When they are not bound or in their natural state, the associated charge is 0. Since Br and F are both diatomic (2 atoms=natural state), their charges are 0. So hydrogen is staying constant, Br is being oxidized and F is being reduced. Hope this helps! Solution Is this a reduction oxidation reaction? If so, what you use is the periodic table. Hydrogen will always have a +1 charge associated with it and Br and F are both halogens which have a -1 charge associated with them. For your reaction, Hydrogen is staying constant at +1 while Br is going from -1 to 0 and F is going from 0 to -1. When atoms are bound to other atoms, they display a charge. When they are not bound or in their natural state, the associated charge is 0. Since Br and F are both diatomic (2 atoms=natural state), their charges are 0. So hydrogen is staying constant, Br is being oxidized and F is being reduced. Hope this helps!.

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Is this a reduction oxidation reaction? If so, what you use is the periodic table. Hydrogen will always have a +1 charge associated with it and Br and F are both halogens which have a -1 charge associated with them. For your reaction, Hydrogen is staying constant at +1 while Br is going from -1 to 0 and F is going from 0 to -1. When atoms are bound to other atoms, they display a charge. When they are not bound or in their natural state, the associated charge is 0. Since Br and F are both diatomic (2 atoms=natural state), their charges are 0. So hydrogen is staying constant, Br is being oxidized and F is being reduced. Hope this helps! Solution Is this a reduction oxidation reaction? If so, what you use is the periodic table. Hydrogen will always have a +1 charge associated with it and Br and F are both halogens which have a -1 charge associated with them. For your reaction, Hydrogen is staying constant at +1 while Br is going from -1 to 0 and F is going from 0 to -1. When atoms are bound to other atoms, they display a charge. When they are not bound or in their natural state, the associated charge is 0. Since Br and F are both diatomic (2 atoms=natural state), their charges are 0. So hydrogen is staying constant, Br is being oxidized and F is being reduced. Hope this helps!

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Is this a reduction oxidation reaction If so, wh.pdf

  • 1. Is this a reduction oxidation reaction? If so, what you use is the periodic table. Hydrogen will always have a +1 charge associated with it and Br and F are both halogens which have a -1 charge associated with them. For your reaction, Hydrogen is staying constant at +1 while Br is going from -1 to 0 and F is going from 0 to -1. When atoms are bound to other atoms, they display a charge. When they are not bound or in their natural state, the associated charge is 0. Since Br and F are both diatomic (2 atoms=natural state), their charges are 0. So hydrogen is staying constant, Br is being oxidized and F is being reduced. Hope this helps! Solution Is this a reduction oxidation reaction? If so, what you use is the periodic table. Hydrogen will always have a +1 charge associated with it and Br and F are both halogens which have a -1 charge associated with them. For your reaction, Hydrogen is staying constant at +1 while Br is going from -1 to 0 and F is going from 0 to -1. When atoms are bound to other atoms, they display a charge. When they are not bound or in their natural state, the associated charge is 0. Since Br and F are both diatomic (2 atoms=natural state), their charges are 0. So hydrogen is staying constant, Br is being oxidized and F is being reduced. Hope this helps!