Periodic Trends And Bonding

Explanation
As you cross a period from left to right on the periodic table, the atomic radius generally decreases. This is because the number of protons in the nucleus increases, causing a stronger attraction between the protons and the electrons. As a result, the electrons are pulled closer to the nucleus, leading to a smaller atomic radius.

Explanation
As you travel down a group in the periodic table, the trend in ionization energy is that it decreases. This is because as you move down a group, the number of energy levels or shells increases. The outermost electrons are further away from the positively charged nucleus, resulting in a weaker attraction between the electrons and the nucleus. Therefore, it requires less energy to remove an electron, leading to a decrease in ionization energy.

Explanation
Metals are located on the left of the stairstep on the periodic table. This is because metals are typically found on the left side of the periodic table and are known for their high electrical conductivity, luster, and malleability. They tend to lose electrons and form positive ions during chemical reactions. The stairstep on the periodic table separates metals from nonmetals, with metals being located to the left and nonmetals to the right.

Explanation
The trend in electronegativity across a period is that it increases. Electronegativity is the measure of an atom's ability to attract electrons towards itself in a chemical bond. As we move across a period from left to right, the number of protons in the nucleus increases, resulting in a stronger positive charge. This increased positive charge attracts electrons more strongly, leading to a higher electronegativity value. Therefore, the electronegativity of elements generally increases as we move across a period.

Explanation
An ionic bond is a type of chemical bond that forms between a metal and a nonmetal. In this type of bond, electrons are transferred from the metal atom to the nonmetal atom, resulting in the formation of positively charged metal ions and negatively charged nonmetal ions. These ions are then attracted to each other due to their opposite charges, creating a strong bond. Therefore, it is true that an ionic bond forms between a metal and a nonmetal.

Explanation
When the difference in electronegativity is low, ions are not formed. Ions are formed when there is a high difference in electronegativity between atoms, causing one atom to attract the shared electrons more strongly and resulting in the formation of positively or negatively charged ions.

Explanation
Covalent compounds are not conductive because they do not have free ions or electrons that can carry an electric current. In covalent compounds, atoms share electrons to form bonds, and these shared electrons are localized between the bonded atoms rather than being free to move throughout the compound. Therefore, covalent compounds do not conduct electricity.

Explanation
The statement "The chloride ion has a negative charge" is correct because chloride ions have gained an electron, resulting in a negative charge. The statement "The hydrogen oxygen bond is covalent" is correct because hydrogen and oxygen share electrons in a covalent bond. The statement "Atoms combine to form a stable octet of valence electrons" is correct because atoms tend to bond with other atoms in order to achieve a full outer shell of electrons, which is often eight electrons.

Explanation
Metallic bonding occurs between metal atoms, not between metals and non-metals. In a metallic bond, the valence electrons are delocalized and form a "sea" of electrons that are free to move throughout the metal lattice. This delocalization of electrons allows metals to conduct electricity and heat well. Therefore, the correct answer is that the electron sea is made of delocalized electrons.