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3 years ago

In a molecule of water, how many electrons are shared between each hydrogen atom and an oxygen atom? A. One B. Two C. Four

Chemistry

2 answers:

lesya692 [45]3 years ago

6 0

The answer is Two (B).

Tems11 [23]3 years ago

6 0

solution:

answer is two

explanation:

In sharing of electrons in the equation water each carbon atom and hydrogen atom share its one electron from its outermost orbit.

since carbon has seven electrons in its outermost orbit and it wants to get one electron to complete its octet.

while hydrogen atoms has one electron to its outermost orbit and it needs one electron to complete its duet.

similarly

second hydrogen atom do as the shame process as it also share one electron to carbon to complete its duet.

after the sharing of electrons both the atoms form molecule water which is stable.

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kari74 [83]

Answer:

I can use a dichotomous key. It helps me classify objects by sorting it out with "yes" and "no" questions.

I can use a Punnett Square. It helps me classify what genes the offspring will receive simply by figuring out the recessive and dominant genes as well as the hetzygous and homzygous.

Now give an example of which ever chart you choose by drawing it if that is required. For the Punnett Square label each of the squares Top right Hetzygous, top left dominant, bottom left recessive, bot-tom right homzygous. And for the dichotomous key put a 5-7 length branch showing the animals that have fur, can breathe under water, what cannot or doesn't have those traits. or something similar

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3 0

3 years ago

Read 2 more answers

Under standard-state conditions, which of the following species is the best reducing agent? a. Ag+ b. Pb c. H2 d. Ag e. Mg2+

eimsori [14]

Answer: The correct answer is Option b.

Explanation:

Reducing agents are defined as the agents which help the other substance to get reduced and itself gets oxidized. They undergo oxidation reaction.

$X\rightarrow X^{n+}+ne^-$

For determination of reducing agents, we will look at the oxidation potentials of the substance. Oxidation potentials can be determined by reversing the standard reduction potentials.

For the given options:

Option a: $Ag^+$

This ion cannot be further oxidized because +1 is the most stable oxidation state of silver.

Option b: $Pb$

This metal can easily get oxidized to $Pb^{2+}$ ion and the standard oxidation potential for this is 0.13 V

$Pb\rightarrow Pb^{2+}+2e^-;E^o_{(Pb/Pb^{2+})}=+0.13V$

Option c: $H_2$

This metal can easily get oxidized to $H^{+}$ ion and the standard oxidation potential for this is 0.0 V

$H_2\rightarrow 2H^++2e^-;E^o_{(H_2/H^{+})}=0.0V$

Option d: $Ag$

This metal can easily get oxidized to $Ag^{+}$ ion and the standard oxidation potential for this is -0.80 V

$Ag\rightarrow Ag^{+}+e^-;E^o_{(Ag/Ag^{+})}=-0.80V$

Option e: $Mg^{2+}$

This ion cannot be further oxidized because +2 is the most stable oxidation state of magnesium.

By looking at the standard oxidation potential of the substances, the substance having highest positive $E^o$ potential will always get oxidized and will undergo oxidation reaction. Thus, considered as strong reducing agent.