Which nuclear emission is negatively charged?(1) an alpha particle
(2) a beta particle
(3) a neutron
(4) a positron

Answers

Answer 1

Answer:

The nuclear emission that is negatively charged is $\boxed{{\text{2}}{\text{. a beta particle}}}$ .

Further Explanation:

Radioactive decay:

Also known as nuclear decay, radioactivity, nuclear or radioactive disintegration. It is the process due to which an unstable atomic nucleus releases its energy in the form of various particles such as alpha particles, beta particles, and gamma particles.

Following are the types of radioactive decays:

1. Alpha decay

In this decay, alpha particles are emitted by unstable nuclei. An alpha particle is a helium nucleus with two protons and two neutrons. It has a charge of +2. The general equation for an alpha decay is as follows:

$_{\text{Z}}^{\text{A}}{\text{X}} \to _{{\text{Z - 2}}}^{{\text{A - 4}}}{\text{X}} + _{\text{2}}^{\text{4}}{\text{He}}$

2. Beta decay

In this decay, beta particles are produced. This occurs when the nucleus decays continuously and emits an electron or a positron. The general equation for beta decay is as follows:

$_{\text{Z}}^{\text{A}}{\text{X}} \to _{{\text{Z + 1}}}^{\text{A}}{\text{X}} + _{{\text{ - 1}}}^{\text{0}}{\beta }}$

Beta decay is further classified as follows:

(a) ${\beta }}^-}$ decay: In this decay, an electron and an electron antineutrino are emitted. The atomic number of the element is increased by one. Its general equation is as follows:

$_{\text{Z}}^{\text{A}}{\text{X}}\to _{{\text{Z+1}}}^{\text{A}}{\text{X}}+{e^-}+{\mathop{\text{v}}\limits^-_{\text{e}}}$

(b) ${\beta }}^+}$ decay or positron emission: In this decay, a positron and an electron neutrino are emitted. The atomic number of the element is decreased by one. Its general equation is as follows:

$_{\text{Z}}^{\text{A}}{\text{X}} \to _{{\text{Z}} - 1}^{\text{A}}{\text{X}}+{e^+}+{{\text{v}}_{\text{e}}}$

3. Gamma decay

In this decay, gamma rays are emitted. Energy is emitted during gamma decay but the number of protons remains unaltered. The general equation for gamma decay is as follows:

$_{\text{Z}}^{\text{A}}{\text{X}} \to _{\text{Z}}^{\text{A}}{\text{X}} + _{\text{0}}^{\text{0}}{{\gamma }}$

4. Neutron emission

It is the type of radioactive decay that occurs when one or more neutrons are ejected from a nucleus. Neutrons are the subatomic particles with no charge. Since only neutrons are removed from the atom, the number of protons as well electrons remain unaltered. This results in the formation of an isotope of the same element.

Therefore the negatively charged nuclear emission is a beta particle because an electron that is a negatively charged species is lost in ${\beta }}^-}$ decay, a type of beta decay.

Learn more:

1. What nuclide will be produced in the given reaction? brainly.com/question/3433940

2. Calculate the nuclear binding energy: brainly.com/question/5822604

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Nuclear chemistry

Keywords: alpha particle, beta particle, gamma decay, positron, negatively charged, neutron emission, radioactivity, radioactive decay, unstable atomic nucleus.

Answer 2

Answer: a beta particle is negatively charged

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2
How many molecules are in 2.47 moles of CC14? *

Answers

Answer:

1.49x10^24 molecules

How many grams of a stock solution that is 92.5 percent H2SO4 by mass would be needed to make 250 grams of a 35.0 percent by mass solution? Show all of the work needed to solve this problem.

Answers

M1m1 = M2m2

where M1 is the concentration of the stock solution, m1 is the mass of the stock solution, M2 is the concentration of the new solution and m2 is its new mass.

M1m1 = M2m2

.925(m1) = .35(250)

m1 = 94.59 g

Answer: 94.59 grams of 92.5 % $H_2SO_4$ by mass solution will be needed.

Explanation:

Mass of sulfuric acid is 250 grams of 35 % by mass solution:

$35=(x)/(250 g)* 100$

$x=87.5 g$

Mass of $H_2SO_4$ in 250 g of 35 % solution = 87.5 g

Mass of 92.5 % $H_2SO_4$ needed to make 35 % by mass solution.

$92.5=\frac{87.5 g}{\text{mass of the solution required}}* 100$

Mass of the solution required = 94.59 g

94.59 grams of 92.5 % $H_2SO_4$ by mass solution will be needed.

The difference in the direction is caused by the ______________.Please help!

Answers

What don’t understand question

Which solution would most likely cause a plant placed in it to become firmer and more rigid? A. hypertonic B. hypotonic C. isotonic D. osmotic

Answers

"Hypotonic" is the one solution among the choices given in the question that would most likely cause a plant placed in it to become firmer and more rigid. The correct option among all the options that are given in the question is the second option or option "B". I hope the answer has come to your great help.

What's at the bottom of a black hole?

Answers

All matter in a black hole is crushed into a single point at the center called singularity.

An unknown compound contains only carbon, hydrogen, and oxygen (cxhyoz). combustion of 3.50 g of this compound produced 5.13 g of carbon dioxide and 2.10 g of water.how many moles of hydrogen, h, were in the original sample?

Answers

The combustion reaction of the unknown compound can be written as follows:

${CxHyOz + O2 → CO2 + H2O}$

Other part of the question is discussed below:

We know that 3.50 g of the compound produced 5.13 g of carbon dioxide and 2.10 g of water. This means that 1.63 g of oxygen were also produced in the reaction.

The mass of oxygen in the original sample is equal to the mass of oxygen produced in the reaction, so the original sample contained 1.63 g of oxygen.

The total mass of carbon and hydrogen in the original sample is equal to the mass of the sample minus the mass of oxygen, which is 3.50 g - 1.63 g = 1.87 g.

We can find the number of moles of hydrogen in the original sample by dividing the mass of hydrogen by the molar mass of hydrogen (1.008 g/mol). This gives us 1.87 g / 1.008 g/mol = 1.86 moles of hydrogen.

Therefore, the answer is 1.86

Learn more about combustion on:

brainly.com/question/34266172

#SPJ12

Final answer:

By dividing the mass of water produced in combustion by the molar mass of Hydrogen in water, we find that the original compound contained 1.05 mol of Hydrogen.

Explanation:

To determine the mole amount of Hydrogen in the compound, you have to consider the reaction applied, and how it applies to the law of conservation of mass. Combustion of the compound produces carbon dioxide (CO2) and water (H2O). For water, one mol equals to the molar mass of H which is 1 g/mol, times the amount of H in water which is 2 to get 2 g/mol. Now knowing that 2.10 g of water were produced from combustion, we divide this by the molar mass of H-in-water to get the number of hydrogen moles in the original sample. So, the calculation will be 2.10 g/ 2 (g/mol) = 1.05 mol. So, the original compound contained 1.05 mol of hydrogen.