Study "chemistry ionic , covalent", a flashcard deck on FORKSAI.
Define ionic bonding and explain how it differs from covalent bonding in terms of electron movement.
Ionic bonding is the strong electrostatic force of attraction between oppositely charged ions, formed when a metal atom transfers one or more electrons to a non-metal atom. In contrast, covalent bonding involves non-metal atoms sharing pairs of electrons between each other, rather than transferring them.
How do metal atoms achieve a full outer shell of electrons when forming an ionic bond?
Metal atoms achieve a full outer shell by losing electrons to form positive ions (cations). This loss of electrons results in the atom having more protons than electrons, giving it a positive charge and a stable electron configuration similar to a noble gas.
Explain why ionic compounds typically have high melting and boiling points.
Ionic compounds have high melting and boiling points due to the strong electrostatic forces of attraction between the oppositely charged ions in their giant ionic lattice structure. A significant amount of energy is required to overcome these strong forces and break down the lattice.
Describe the formation of a chloride ion (Cl-) from a chlorine atom, including the change in electron count and charge.
A chlorine atom, being a Group 7 non-metal, gains one electron to achieve a full outer shell. This gain of an electron results in the formation of a negative chloride ion (Cl-), as it now has one more electron than protons.
Why are intermolecular forces not considered chemical bonds?
Intermolecular forces are not considered chemical bonds because they do not involve the transfer or sharing of electrons, and no new compounds are formed. They are typically much weaker, around one-tenth the strength of a chemical bond.
How does the group number of an element relate to the charge on the ion it forms in an ionic bond?
The group number of an element directly relates to the charge on the ion it forms. For example, Group 1 metals form 1+ ions, Group 2 metals form 2+ ions, Group 6 non-metals form 2- ions, and Group 7 non-metals form 1- ions, as they gain or lose electrons to achieve a noble gas electronic structure.
Explain the primary limitation of a 3D ball and stick model when representing an ionic lattice structure.
A primary limitation of the 3D ball and stick model is that it incorrectly depicts space existing between individual ions, representing ionic bonds as sticks. In reality, an ionic bond is an electrostatic force of attraction that acts in all directions around an ion, and there is not much space between separate ions.
Why do simple covalent molecules not conduct electricity?
Simple covalent molecules do not conduct electricity because they do not contain free electrons or ions that are able to move and carry an electric charge. The electrons are held in fixed positions within the covalent bonds.
What is the role of delocalised electrons in metallic bonding?
In metallic bonding, delocalised electrons are electrons from the outer shells of metal atoms that are free to move throughout the entire metallic lattice structure. They form a 'sea of electrons' which creates strong electrostatic attractions with the positive metal ions, holding the structure together.
Distinguish between bonding electrons and non-bonding electrons in a covalent molecule.
Bonding electrons are the pairs of electrons that are shared between two atoms to form a covalent bond. Non-bonding electrons, also known as lone pairs, are electrons on the outer shell of an atom that are not involved in forming covalent bonds.