Unit 1 Higher Chemistry Flashcards
What’s the trend for covalent radius across a period?
As you move across a period the number of protons increases which increases nuclear charge. Each new electron is added to the same shell, as the nuclear charge increases the electrons are pulled and closer. This decreases the size of the atom.
What’s the trend for covalent radius down a group?
as you move down a group the number of protons increases, which increases nuclear charge. However the number of occupied energy levels also increases. These energy levels shield the electrons from the nuclear charge. The more energy levels, the greater the shielding and the bigger the atoms will be.
What’s the trend for ionization energy across a period?
as you move across a period in the number of protons increases, which increases nuclear charge. Each new electron is added to the same shell, as the nuclear charge increases the electrons are pulling closer. This makes it harder to remove an electron so I know an energy increases.
What is the trend for ionization energy down a group?
As you move down a group the number of protons increases, which increases nuclear charge.however the number of occupied energy levels also increases. These energy levels also increase. These energy levels shield the electrons from nuclear charge. The more energy levels, the greater the shielding effect and the easier it is to remove an electron so energy decreases.
What is the trend for electronegativity across a period?
As you move across a period of the number of protons increases, which increases nuclear charge. Each new electron is added to the same show, as the nuclear charge increases the attraction the atom has for its a bonding electrons increases. So electronegativity increases.
What is the trend for electronegativity down a group?
As you move down a group the number of protons increases, which increases nuclear charge. However the number of occupied energy levels also increases. These energy levels shield the electrons from the nuclear charge. The more energy levels, the greater the shielding effect and the less attraction the nucleus has for its bonding electrons. Electronegativity decreases.
