Survey
* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
The Periodic Table Unit 4 Page 4 Learning Target: I can use the Periodic Table to identify and explain periodic trends, including atomic and ionic radii, electronegativity, and ionization energy. Criteria For Success: I can explain effective nuclear charge and electron shielding. I can explain how increasing effective nuclear charge across a period influences the atomic radius, electronegativity and ionization energy. I can explain how increased electron shielding down a group influences atomic radius, electronegativity and ionization energy. I can explain the trend of ionic radius and how the magnitude and the sign of the ionic charge influences ionic radius Notes: Periodic Trends A. Attraction between the nucleus and electrons 1. Coulomb’s law- the force of attraction between two _________________ charged particles is ______________ proportional to the magnitude of the charges and __________________ proportional to the distance between those charges. 𝑘𝑞1 𝑞2 𝐹= 𝑟2 2. Effective nuclear charge (Zeff)- the net _______________ _________ experienced by the _______________ electrons in an atom. a. Zeff = # protons - # core (non-valence) electrons 3. Electron shielding- the inner electrons ______________ the outer electrons from some of the nucleus’ ___________________ force. a. Going down a group adds another ___________________ energy level adds more shielding. B. Periodic trends are _________________ in the periodic table relating to the ________ and other ________________ of elements. 1. ATOMIC RADIUS is the ________________ between the nucleus and the ____________ edge of the electron cloud. 2. IONIZATION ENERGY is the _____________ required to _________________ an electron from the atom. a. Each additional electron requires ___________ energy to remove than the previous one, so the ________________ ionization energy will be greater than the __________ ionization energy, and so on. c. EXCEPTIONS: i. O vs. N- It’s easier to remove an electron from O because of the ________________ of the paired electrons. ii. Be vs. B- It’s easier to remove an electron from B because it’s a __________________ vs. an ____________________ and electrons in p orbitals are held less _________________. 3. ELECTRONEGATIVITY is the ability of an atom in a __________________ [meaning it’s participating in a ___________] to attract _________________ electrons to itself. a. Think of the atoms as playing “tug of war” with their ____________ shell electrons. 4. IONIC RADIUS is the ________________ from the nucleus to the outer edge of the electron cloud in a ________________ ion. a. Cation- the atom __________ electron(s), has a ________________ charge b. Anion- the atom ______________ electron(s), has a ________________ charge c. All atoms want a __________ valence shell, and will gain/lose electrons to get there. The Periodic Table Unit 4 Page 5 Draw arrows representing the trend of each of the following from decreasing to increasing: Electronegativity, atomic radius, Ionizations energy, electron affinity, reactivity 1. Organize the following elements in order of decreasing to increasing for each property: Mg, S, Fr, F, Al, Zn Electronegativity: Atomic radius: Ionization energy: Electron affinity: 2. What happens to atomic radius as you go across a period? Why does this happen? 3. What happens to reactivity as you go down a group? Why does this happen? Organize the following in increasing reactivity: Be, Ca, Ba, Mg, Ra, Sr. 4. Why does an electron increase in electronegativity as it moves across the periodic table? 5. How does electron shielding contribute to the trend of increasing reactivity as you go down a group for metals? How does it contribute the trend of increasing reactivity as you go up a group for non-metals?