OPENER: 9/14 and 9/15 Periodic Trends
Quiz by Darrien James
Feel free to use or edit a copy
includes Teacher and Student dashboards
Measure skillsfrom any curriculum
Tag the questions with any skills you have. Your dashboard will track each student's mastery of each skill.
- edit the questions
- save a copy for later
- start a class game
- automatically assign follow-up activities based on students’ scores
- assign as homework
- share a link with colleagues
- print as a bubble sheet
- Q1
Which of the following best explains the difference in ionization energy between Cesium (Cs) and Sodium (Na)?
Sodium has a higher ionization energy than Cesium because it has a smaller atomic radius and the valence electron is closer to the nucleus therefore the attraction between the positively charged nucleus and the negatively charged valence electron is stronger therefore more energy is required to remove the valence electron.
Cesiumhas a higher ionization energy than Sodium because it has a larger atomicradius and the valence electron is further away from the nucleus therefore theattraction between the positively charged nucleus and the negatively chargedvalence electron is weaker therefore more energy is required to remove the valenceelectron.
Cesium has a lower ionization energy than Sodium because it is has a smaller atomic radius and the valence electron electron is closer to the nucleus therefore the attraction between the positively charged nucleus and the negatively charged valence electron is stronger therefore less energy is required to removed the valence electron.
Cesium has a lower ionization energy than Sodium because it is has a smaller atomic radius and the valence electron electron is closer to the nucleus therefore the attraction between the positively charged nucleus and the negatively charged valence electron is weaker therefore less energy is required to removed the valence electron.
30s - Q2
Arrange the following elements in order of increasing atomic radius:
Li, K, Rb, Na
Na, K, Rb, Li
Rb, K, Na, Li
Li, K, Na, Rb
Li, Na, K, Rb
30s - Q3
Arrange the following in order of increasing electronegativity:
Si, Cl, F, K, Ca
F, Cl, Si, Ca, K
Si, Cl, Ca, F, K
K, Ca, Si, Cl, F
K, Ca, Cl, Si, F
30s - Q4
Define electronegativity:
The ability of an atom to pull electrons toward itself in a bond.
The amount of energy required to remove an electron from an atom.
The size of an atom.
It is the total charge of the electrons.
30s - Q5
Which of the following elements have similar chemical properties, Explain?
He, Zn, and Mg, because they are in the same group.
F, Cl, and Br, because they are in the same group.
K, Ga, and Kr because they are in the same group.
C, N, and O, because they are in the same period.
30s