Atoms and Atomic Structure

No, sulfur does not have a full valence shell. It has six valence electrons and needs two more to achieve a full octet, which consists of eight electrons. In chemical reactions, sulfur typically forms compounds by gaining, losing, or sharing electrons to complete its valence shell.

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The maximum number of electrons in the first energy shell of an atom is 2. This limitation is due to the shell's capacity to accommodate a maximum of one s orbital, which can hold a maximum of two electrons, each with opposite spins.

Bonded atoms are generally more chemically stable than unbonded neutral atoms because they achieve a lower energy state through the formation of chemical bonds, which allows them to fill their valence electron shells. This "octet rule" leads to a more stable electron configuration, reducing reactivity. In contrast, unbonded neutral atoms often have incomplete valence shells, making them more prone to reactions as they seek to achieve stability through bonding. Thus, the bonding process stabilizes atoms by overcoming their inherent tendency to react.

By definition, Avogadro's Number, about 6.022 X 1023, for an element is the number of atoms in one gram atomic mass. The gram atomic mass of silver is 107.868. Therefore, the mass of 5.44 X 1025 atoms of silver is [(5.44 X 1025)/(6.022 X 1023)] X 107.868 or 974 grams, to the justified number of significant digits.

The atomic radius of an anion increases compared to its neutral atom because the addition of one or more electrons leads to increased electron-electron repulsion within the electron cloud. This repulsion causes the electrons to spread out more, resulting in a larger atomic radius. Additionally, the effective nuclear charge experienced by the outer electrons may decrease due to the increased shielding effect, further contributing to the expansion of the atomic size.

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No, negative charge does not have more magnitude than positive charge; both types of charge are equal in magnitude but opposite in sign. The unit of charge, the coulomb, applies equally to both positive and negative charges. Therefore, a negative charge of -1 coulomb has the same magnitude as a positive charge of +1 coulomb, just with an opposite sign.

Hydrogen nuclei, which consist of single protons, can combine through nuclear fusion to form helium nuclei under extreme temperatures and pressures, such as those found in the cores of stars. During this process, two hydrogen nuclei (protons) can fuse to create deuterium (a hydrogen isotope), releasing positrons and neutrinos. Additional reactions can then convert deuterium and protons into helium-3 and ultimately helium-4. This fusion process releases a significant amount of energy, which powers stars and produces light.

An atom with 34 protons in its nucleus is an atom of the element selenium (Se). The number of protons determines the atomic number, and selenium has an atomic number of 34 on the periodic table.

To determine the number of electrons lost or gained by elements forming ions that obey the octet rule, we can refer to their positions in the periodic table. Metals, such as sodium (Na), typically lose one electron to achieve a stable electron configuration, while nonmetals, like chlorine (Cl), gain one electron to complete their outer shell. For example, sodium loses 1 electron to form Na⁺, and chlorine gains 1 electron to form Cl⁻. Thus, metals generally lose electrons, and nonmetals gain electrons to achieve stability.

You appear to misunderstand.

A charged atom is named an ION. It is NOT an atom.

An atom of any element has a given number of protons.

That same atom when it becomes an ion still contains the same number of protons.

The difference between an atom and an ion is the number of electrons surrounding the nucleus.

e.g.

Sodium

An atom of Sodium contains 11 protons and 11 electrons ; Symbol (Na)

An ion of Sodium contains 11 protons and 10 electrons ; Symbol (Na^(+)).

Note the same number of protons , but a different number of electrons.

NNB If an atom of an element , gains of loses protons, then it becomes a different element. This involves a nuclear reactor; not a chemistry lab.

e.g.

Hydrogen ; 1 proton

Helium ; 2 protons.

An atom, of any element, has three different particles in its construction. They are protons, Neutrons and electrons.

The protons are positively(+) charged, the neutrons have no charge, and the electrons have negative(-) charge.

The protons and neutrons are found un the nucleus of the atom, and are collectively named as nucleons. The electrons are found in energy shells surrounding and outside the nucleus.

Any one element has its own characteristic number of protons and electrons.

Taking carbon as an example. It has six(6) protons and six(6) electrons.

As another example, oxygen has eight( 8) protons and eight (8) electrons.

et.seq.,

Protons and Electrons.

Protons are positively)+) charged and electrons (-) are negatively charged.

For an atom to be neutrally charged the number of protons MUST equal the number of electrons. The number of positives must equal the number of negatives.

When these number are NOT equal ; loss/gain of electrons, then the atom is named an ION.

Definitively ' an Isotope has a different number of neutrons'.

Most elements exhibit isotopes.

However, for hydrogen , it has three isotopes.

#1 protium ; 1 proton, 0 neutrons , 1 electron (The commonest isotope)

#2 deuterium ; 1 proton. 1 neutron, 1 electron ( heavy hydrogen_

#3 tritium ; 1 proton , 2 neutrons , 1 electron ( super heavy hydrogen/radio-active).

Notice in each case that the number of neutrons varies, but the other particles remain the same.

When inspecting the Periodic Table, you will find two number against each element.

The smaller number is the Atomic Number and also the number of protons in the element.

The larger number is the Atomic Mass , which is the total of all the protons and neutrons in that element.

Hence to find the number of neutrons in an element.

Subtract Atomic Mass from Atomic Number.= number of neutrons.

The total number of subatomic particles in the nucleus is the sum of protons and neutrons. For the common isotope of iron with an atomic number of 26, there are 26 protons. Given the mass number of 56, the number of neutrons can be calculated as 56 - 26 = 30. Therefore, the total number of subatomic particles in the nucleus is 26 protons + 30 neutrons = 56 particles.

An atom has the same number of electrons and protons. Protons are positively charged particles found in the nucleus of an atom, while electrons are negatively charged particles that orbit the nucleus.

One where the number of protons (+) equal the number of electrons (-).

one were the proton cancels out the electrons Ex. -5 +5 makes 0 uncharged atoms

Electrons are organized in atoms into specific energy levels or shells, which are further divided into sublevels and orbitals. The arrangement follows the principles of quantum mechanics, with electrons occupying the lowest available energy states first (the Aufbau principle) and adhering to the Pauli exclusion principle, which states that no two electrons can have the same set of quantum numbers. The organization of electrons determines an element's chemical properties and its behavior in bonding and reactions.

The chemical that shows the relative number of atoms of each element in a compound is called a chemical formula. A chemical formula provides a concise representation of a compound, indicating the types and quantities of atoms present, typically using symbols for the elements along with subscripts to denote the number of each type of atom. For example, the formula ( \text{H}_2\text{O} ) indicates that each molecule of water contains two hydrogen atoms and one oxygen atom.

An iron-56 nucleus (⁵⁶Fe) must absorb 19 neutrons to produce an arsenic-75 nucleus (⁷⁵As). This can be represented by the nuclear equation:

[ ^{56}{26}Fe + 19 , ^1_0n \rightarrow ^{75}{33}As + 2 , ^4_2He ]

This equation shows that the absorption of 19 neutrons and the ejection of 2 helium nuclei (alpha particles) results in the formation of arsenic-75.

When atoms combine to form molecules, a synthesis reaction occurs, where simpler substances unite to create more complex compounds. Conversely, when molecules break down into atoms, a decomposition reaction takes place, involving the breakdown of a compound into its constituent elements or simpler compounds. Both types of reactions involve changes in chemical bonds and are fundamental processes in chemistry.

J.J. Thomson's discovery of the electron in 1897 marked a pivotal moment in atomic physics, revealing that atoms are not indivisible but composed of smaller particles. His experiments demonstrated that electrons are negatively charged and much lighter than atoms, leading to the realization that atoms contain subatomic particles. This discovery laid the groundwork for the development of the modern atomic model and profoundly influenced the fields of chemistry and physics. Additionally, Thomson's work paved the way for further research into atomic structure, ultimately leading to the development of quantum mechanics.

The reaction between sodium thiosulfate (Na2S2O3) and chlorine (Cl2) can be represented by the equation:

[ \text{Cl}_2 + 2 \text{Na}_2\text{S}_2\text{O}_3 \rightarrow 2 \text{NaCl} + \text{Na}_2\text{S}_4\text{O}_6 ]

From the balanced equation, 1 mole of Cl2 reacts with 2 moles of Na2S2O3. Therefore, to react with 0.12 moles of Cl2, you would need 0.12 moles × 2 = 0.24 moles of Na2S2O3.