d. I Lead, 2 Nitrogen, 2 Oxygen
7. Number of neutrons are calculated by taking difference of
8. The fourth shell is
shell. It can accommodate only
and
electrons.
Answers
Answer:
In chemistry and atomic physics, an electron shell may be thought of as an orbit followed by electrons around an atom's nucleus. The closest shell to the nucleus is called the "1 shell" (also called the "K shell"), followed by the "2 shell" (or "L shell"), then the "3 shell" (or "M shell"), and so on farther and farther from the nucleus. The shells correspond to the principal quantum numbers (n = 1, 2, 3, 4 ...) or are labeled alphabetically with the letters used in X-ray notation (K, L, M, …).
Each shell can contain only a fixed number of electrons: The first shell can hold up to two electrons, the second shell can hold up to eight (2 + 6) electrons, the third shell can hold up to 18 (2 + 6 + 10) and so on. The general formula is that the nth shell can in principle hold up to 2(n2) electrons.[1] For an explanation of why electrons exist in these shells see electron configuration.[2]
Each shell consists of one or more subshells, and each subshell consists of one or more atomic orbitals.
Answer:
All atoms except hydrogen are multiple-electron atoms. The physical and chemical properties of elements are directly related to the number of electrons a neutral atom has. The periodic table of the elements groups elements with similar properties into columns. This systematic organization is related to the number of electrons in a neutral atom, called the atomic number, Z. We shall see in this section that the exclusion principle is key to the underlying explanations, and that it applies far beyond the realm of atomic physics.
In 1925, the Austrian physicist Wolfgang Pauli (see Figure 1) proposed the following rule: No two electrons can have the same set of quantum numbers. That is, no two electrons can be in the same state. This statement is known as the Pauli exclusion principle, because it excludes electrons from being in the same state. The Pauli exclusion principle is extremely powerful and very broadly applicable. It applies to any identical particles with half-integral intrinsic spin—that is, having s = 1/2, 3/2, … Thus no two electrons can have the same set of quantum numbers.
Explanation:
Atoms are the basic unit of chemistry. They are composed of three basic parts:
1) Neutrons: Neutrons are uncharged particles that are found in the center of the atom (the nucleus). Neutrons give mass (weight) to the atom but do not participate in chemical reactions.
2) Protons: Protons are positively charged particles that are also found in the nucleus. Like neutrons, protons give mass to the atom but do not participate in chemical reactions. The number of protons an atom has is called the atom’s atomic number, and determines the atom’s identity (e.g. carbon atoms have 6 protons, oxygen atoms have 8 protons).
3) Electrons: Electrons are negatively charged particles that are found in electron shells surrounding the nucleus. They have essentially no mass but are important in chemical reactions. The first electron shell can hold 2 electrons. For most biologically relevant atoms, additional electron shells (if present) can hold up to eight electrons.
Each atom contains equal numbers of protons and electrons. The number of neutrons may vary within atoms of a particular type. (For example, carbon atoms may have 6, 7, or 8 neutrons). Atoms that vary only in the number of neutrons are called isotopes.
Bonds
Atomic stability:
The stability of atoms depends on whether or not their outer-most shell is filled with electrons. If the outer shell is filled, the atom is stable. Atoms with unfilled outer shells are unstable, and will usually form chemical bonds with other atoms to achieve stability.
Example of an unstable atom with a single electron in its outer-most shell.
Example of an unstable atom with 7 electrons in its outer-most shell.
Examples of stable atoms.
The two types of chemical bonds that atoms can form to achieve stability are called ionic bonds and covalent bonds. In ionic bonds, atoms donate or receive electrons to achieve stability. In covalent bonds, atoms share electrons to achieve stability. The type(s) of bond a particular atom can form depends on the numbers of electrons in their outer shells.
Ionic bonds:
Ionic bonds result from the transfer of electrons between atoms. If an atom has only a few electrons in its outer shell, it can achieve stability by donating these electrons to an atom that has an outer shell that is almost full.
For example:
An atom of sodium has only one electron in its outer shell. An atom of chlorine has seven outer electrons (almost a full shell).
If the lone sodium outer electron is transferred to the chlorine atom, both atoms would have full outer shells and so would achieve stability.
When clorine gains an extra electron, it is called chloride.
Since chlorine gained a negatively charged electron, it now has more electrons than protons and has a net negative charge. Since sodium lost an electron, it now has more protons than electrons and so has a net positive charge. Charged particles (like sodium and chlorine after the transfer of electrons) are called ions. (Specifically, positively charged ions are called cations and negatively charged ions are called anions). Due to the opposite charge of the two ions (negative chloride and positive sodium), the two ions are attracted to each other and form an ionic bond. The resulting compound is referred to as an ionic compound. Note that ionic compounds have totally different properties than either of the atoms that make them up. Sodium is a highly reactive silver metal. Chlorine is a toxic green gas. Sodium chloride is table salt.
The animation below further illustrates the formation of the ionic compound sodium chloride.
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