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3 years ago

Which of the following correctly identifies the composition of an oxygen atom?

2 answers:

7 0

Oxygen has the atomic number 8, which eliminates options B and D right away. Any neutral atom, including the oxygen atom, has the same number of protons and electrons, meaning the number of electrons is also 8. If you're still not sold, the oxygen atom has a mass number of 16, which is the sum of the protons and neutrons in the atom, meaning there have to be 8 neutrons as well. The answer is option A.

aleksandrvk [35]3 years ago

3 0

The composition of an oxygen atom is: A) 8 protons, 8 electrons, and 8 neutrons.

<h3>Further Explanation</h3>

To determine how many of the subatomic particles are in the atom, the atomic number is used.

Atomic number is the number that gives the atom its identity and can be found in the periodic table. It gives the number of protons in an atom. It can be observed that the atomic number of the elements are increasing by one unit as you go from left to right.

<em>The atomic number of oxygen is 8, therefore, it has 8 protons.</em>

<em>In a neutral (uncharged atom), the number of protons and electrons are equal.</em>

<em>Hence, oxygen also has 8 electrons.</em>

In the most simple periodic table of elements, the atomic number is usually the smaller number written in the tile for each element. The larger number is the mass number.

The difference between the larger mass number and the smaller atomic number is the number of neutrons:

<em>Number of Neutrons = Mass Number - Atomic Number</em>

The mass number of oxygen is 16. We can use the atomic number and the mass number to get the number of neutrons using the equation above:

<em>Number of Neutrons = 16 – 8</em>

<em>Number of Neutrons = 8</em>

Therefore, it has been determined that the an oxygen atom has 8 protons, 8 electrons and 8 neutrons.

<h3>Learn More</h3>

Periodic Table brainly.com/question/2376134

Isotopes brainly.com/question/2757829

<h3>Keywords: protons, neutrons, electrons, mass number, atomic number</h3>

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VladimirAG [237]

<u>Thorium series</u> could start by this sequence.

<h3>Brief explanation</h3>

To write balanced equations for nuclear decay processes. It's important to remember that the mass number and the atomic numbers must be balanced. And so what that means is that if we look at an elements nuclear symbol, the atomic number is the bottom number and the top number, the superscript, is the mass number, and so when we add them up on both sides, they have to be equal. There are two different ways in which decay can occur.

In this, series one is through beta decay, which means that the following particle is produced. The other is Alpha Decay, which produces this particle. Both are products. So if we start off with uranium to 39 you read it in nuclear notation, which means we have to find the atomic number just 92 and it undergoes beta decay.

So that means that it produces this particle find the second particle we used the atomic number, so 92 equals minus one plus x, where X equals 93 which is Neptune IAM. The mass number of our new isotope is zero plus X equals to 39 where X equals to 39. This product becomes the reactant in my next decay, which is also a beta decay. And to find the unknown element we do the same here.

Except for that it's 93 equals minus one plus x, where X is 94 which is P u plutonium, and the mass number is zero plus X equals to 39 or to 39. The next decay starts with the isotope that we just form to 39 p. U. This time it's an Alpha decay. So we produce this particle to find the unknown. Element 94 equals two plus x, where X equals 92 which takes us back to uranium.

Find the mass number of this isotope 2 39 equals four plus X, where X equals to 35. Finally, for the last decay, you have another Alpha decay starting with uranium to 35 making an alpha particle. The atomic number will be 90 which is T H and the top is 2 31 For the mass number. This begins the natural decay, series of thorium .

Learn more about chemical decay

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1 year ago

Suppose you were preparing 1.0 L of a bleaching solution in a volumetric flask, and it calls for 0.21 mol of NaOCl. If all you h

yulyashka [42]

Answer:

0.256 L

Explanation:

We should use the following formula:

concentration (1) × volume (1) = concentration (2) × volume (2)

concentration (1) = 0.82 M NaOCl

volume (1) = ?

concentration (2) = 0.21 M NaOCl

volume (2) = 1 L

volume (1) = [concentration (2) × volume (2)] / concentration (1)

volume (1) = [0.21 / 1] / 0.82 = 0.256 L

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3 years ago

Read 2 more answers

Enter a molecular equation for the gas-evolution reaction that occurs when aqueous hydroiodic acid and aqueous potassium sulfite

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Answer:

2HI + K2SO3=>2KI+H2SO3

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3 years ago

2. What ions are present in what ratio in a solution of aqueous calcium chloride?

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Answer:

$\mathrm{Ca}^{2+} \text { and } \mathrm{Cl} \text { - ions are present in } 1: 2 \text { ratio in a solution of aqueous calcium chloride. }$

Explanation:

Here in Calcium Chloride ionic bond is present in between calcium and chlorine atoms. As we know according to Octet rule calcium have two excess atoms and for matching nearest noble gas electronic configuration. It donate two electrons to gain more stability and form $\mathrm{Ca}^{2+}$ , while chlorine is deficient from one electron to meet nearest noble gas electronic configuration therefore two chlorine atoms accept excess electron from calcium individually and form two $\mathrm{Cl}^{-}$ ions.

$\text { Equation is as follows: } \mathrm{Ca}^{2+}+2 \mathrm{Cl}^{-} \rightarrow \mathrm{CaCl}_{2}$

Hence aqueous solution of calcium chloride breaks the ionic bond pairing in one $\mathrm{Ca}^{2+}$ and two $\mathrm{Cl}^{-}$ ions: $\mathrm{CaCl}_{2} \longrightarrow \mathrm{H}_{2} \mathrm{O} \quad \mathrm{Ca}^{2+}(\mathrm{ag})+2 \mathrm{Cl}(\mathrm{ag})$

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