Accel-Unit 2- Periodic Table & Electrons

What do the periods on the periodic table tell you?

• electrons
• sublevels
• energy levels

Tags

NGSS.HS-PS1-1

What do the elements in the same group have in common?

• properties & valence electrons
• energy level & valence electrons
• protons & valence electrons

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Ionization Energy is 

• the energy required to remove an electron
• the ability to attract electrons
• half the distance between the nuclei of 2 adjacent atoms
• half the distance between the nuclei of 2 ions

What happens to the radius of an atom when it becomes a cation?

• gets bigger because less electrons, so less electron repulsion
• gets smaller because less electrons, so less electron repulsion
• gets bigger because more electrons, so more electron repulsion
• gets smaller because more electrons, so more electron repulsion

What happens to the radius of an atom when it becomes an anion?

• gets bigger because less electrons, so less electron repulsion
• gets smaller because less electrons, so less electron repulsion
• gets bigger because more electrons, so more electron repulsion
• gets smaller because more electrons, so more electron repulsion

Atomic radius ______ left to right across a period and ______ down a group

• decreases, increases
• increases, decreases

Electronegativity is

• the energy required to remove an electron
• the ability to attract electrons
• half the distance between the nuclei of 2 adjacent atoms
• half the distance between the nuclei of 2 ions

Atomic radius _________ across a period because __________.

• decreases; energy levels and electron shielding increases

• decreases; nuclear charge (more protons) increases

• increases; energy levels and electron shielding increases

• increases; nuclear charge (more protons) increases

Tags

NGSS.HS-PS1-1

Put the elements below in order of increasing ionization energy:  K, Ti, Cs

• Cs, Ti, K
• Ti, K, Cs
• Cs, K, Ti
• Ti, K, Cs

What happens to the atomic radius as you go down a group? 

• gets smaller because the effective nuclear charge gets bigger
• gets bigger because the effective nuclear charge gets smaller
• gets smaller because of an increase in electron shielding
• gets bigger because of an increase in electron shielding