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3 years ago

How does an electron move from the ground state to an excited state?

Chemistry

1 answer:

mrs_skeptik [129]3 years ago

3 0

Answer:

It goes through a process called absorption. This is when an atom absorbs the energy from its surroundings. The electrons move from the ground state to the excited state because of this process. Once the atoms absorb energy, that affects the inner development when shifting to a new state of being.

Explanation:

The process that is known as absorption is when an atom absorbs energy from its surrounding racing it's energy level causing it to go into an excited state or highly-reactive state. When an atom goes through this process, electrons absorb the energy and raise to higher energy levels, therefore raising the stage of itself. This is how it gets into a excited state.

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An atomic number stands for the number of _____. neutrons in the nucleus of an atom protons in the nucleus of an atom valence el

Effectus [21]

Answer:

atoms or electrons

Explanation:

but l guess electrons is the best answer

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3 years ago

Explain how you would determine the amount of g in 1.7 mol of Al(OH)2 and give your answer.

krok68 [10]

Answer:

103.7 grams

Explanation:

$Al(OH)_{2}$

Al: 1 * 26.98 = 26.98

O: 2 * 16.00 = 32.00

H: 2 * 1.01 = 2.02

26.98 + 32.00 + 2.02 = 61.00

$\frac{1.7mol}{1}$ * $\frac{61.00g}{1mol}$ = 103.7 grams of $Al(OH)_{2}$

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3 years ago

What is bias in an experiment?

baherus [9]

Answer:

Explanation:

It pushes the experimental results one way or another. Less reliable.

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3 years ago

Which pairing below does not correctly match the scientist with the contribution to the understanding of the atom? A. Proust and

Lyrx [107]

The answer would be C. In fact, letter A already defines the Law of Definite Proportions. On the other hand, J.J. Thomson was responsible for the discovery of electrons through cathode ray tube experiments. The rest of the choices are true.

5 0

4 years ago

Read 2 more answers

A 1.25-g sample contains some of the very reactive compound al(c6h5)3. on treating the compound with aqueous hcl, 0.951 g of c6h

velikii [3]

<span>83.9% is the weight percent of Al(C6H5)3 in the original 1.25 g sample. First, look up the atomic weights of all elements involved. Atomic weight of Aluminum = 26.981539 Atomic weight of Carbon = 12.0107 Atomic weight of Chlorine = 35.453 Atomic weight of Hydrogen = 1.00794 Now calculate the molar mass of Al(C6H5)3, and C6H6 Molar mass Al(C6H5)3 = 26.981539 + 18 * 12.0107 + 15 * 15.999 = 258.293239 g/mol Molar mass of C6H6 = 6 * 12.0107 + 6 * 1.00794 = 78.11184 g/mol Determine how many moles of C6H6 was produced 0.951 g / 78.11184 g/mol = 0.012174851 mol Since the balanced formula indicates that 3 moles of C6H6 is produced for each mole of Al(C6H5)3 used, divide by 3 to get the number of moles of Al(C6H5)3 that was present. 0.012174851 mol / 3 = 0.004058284 mol Now multiply by the molar mass of Al(C6H5)3 to get the mass of Al(C6H5)3 originally present. 0.004058284 mol * 258.293239 g/mol = 1.048227218 g Finally, divide the mass of Al(C6H5)3 by the total mass of the original sample to get the weight percentage. 1.048227218 g / 1.25 g = 0.838582 Since all our measurements had 3 significant figures, round the result to 3 significant figures, giving 0.839 = 83.9%</span>

4 0

4 years ago