Why certain elements bond well while others do not?
Which of the three sub-atomic particles(electrons, protons, and neutrons) determines most of the properties of an element and why?
How the atom of one element is different from the atom of another element?
I don't understand part 1 about bonding well. I don't know what that means. There are covalent bonds,ionic bonds, metallic bonds, etc.
Part 2. What kind of properties? Chemical or physical? I assume you mean chemical properties. The electrons are involved in bonding; therefore, the electrons and their arrangement in the outside shells are major factors in determining the CHEMICAL properties of elements.
Part 3. Atoms of one element are different from another by the number of protons and the number and arrangement of electrons.
the first part applies with the polar and nonpolar...so why polar and polar bonds better than polar with nonpolar?
I'm not even sure I agree that there is such a thing as a polar atom. We think of polar and non-polar BONDS as being formed between atoms with some difference in electronegativity (for polar bonds) and little or no difference in electronegativity (for non-polar bonds).
I'm I don't see how what makes silver and gold different
Why certain elements bond well while others do not:
The ability of elements to bond with one another is determined by their electron configuration, which refers to the arrangement of electrons in the energy levels or shells around the atomic nucleus.
Elements that have a full outermost energy level (valence shell) tend to be stable and do not easily bond with other elements. These elements are called noble gases, and they include helium, neon, argon, and others. Since their outermost energy level is already complete, they do not have a strong tendency to gain or lose electrons, making them less reactive.
On the other hand, elements that do not have a full outer energy level tend to be more reactive and readily bond with other elements in order to achieve a stable electron configuration. These elements gain, lose, or share electrons to attain a complete outermost energy level. For example, elements in Group 1 of the periodic table, such as lithium, sodium, and potassium, have one electron in their outermost energy level. They lose this electron to achieve a stable configuration.
Bonding between elements occurs through either ionic or covalent bonds. In an ionic bond, one element donates electrons to another, resulting in the formation of positively and negatively charged ions that attract each other. In a covalent bond, elements share electrons, which can create stable electron configurations for both elements involved.
Which of the three sub-atomic particles determines most of the properties of an element and why:
Electrons determine most of the properties of an element. They have a negative charge and are located in the electron shells around the atomic nucleus. The behavior and arrangement of electrons play a crucial role in chemical bonding and the characteristic properties of elements.
The number of electrons in the outermost energy level or valence shell determines an element's reactivity and its tendency to bond with other elements. Elements in the same group on the periodic table have the same number of valence electrons and exhibit similar chemical behavior.
The interaction of valence electrons between atoms determines the type of bonding that takes place. For example, elements with one or two valence electrons tend to lose them and form positive ions. Elements with five, six, or seven valence electrons tend to gain electrons to achieve a stable configuration, forming negative ions. The behavior of electrons in bonding determines the formation of various compounds, such as salts, acids, and bases.
How the atom of one element is different from the atom of another element:
The atom of one element is different from the atom of another element primarily based on the number of protons in the atomic nucleus. Protons are positively charged subatomic particles that determine the atomic number of an element and define its identity.
Each element has a unique number of protons, which is known as its atomic number and is represented in the periodic table. For example, hydrogen has one proton in its nucleus, while carbon has six protons. The atomic number defines the element and differentiates it from others on the periodic table.
In addition to protons, atoms also contain neutrons and electrons. Neutrons are particles with no charge found in the atomic nucleus. They contribute to the mass of the atom but do not significantly affect its chemical behavior. Electrons, on the other hand, are negatively charged particles that orbit the nucleus in energy levels or electron shells.
While the number of protons defines the element, the number of neutrons and electrons can vary within an element, resulting in different isotopes and ions. Isotopes have the same number of protons but different numbers of neutrons, leading to slight differences in atomic mass. Ions are atoms that gain or lose electrons, resulting in a different number of electrons compared to protons and a net electrical charge. However, the essential characteristic that distinguishes one element from another is the number of protons present in its atomic nucleus.