Periodicity

As you move down the periodic table atoms get bigger.  This is because ____________.

• The atoms have more mass.
• The atoms have more protons.
• The atoms have more electron shells

• The atoms have more nuetrons

Electronegativity is...

• how good an atom is at attracting shared electrons

• the ability of an atom to lose electrons
• the energy required to remove an electron from a specific atom
• how easy it is to make friends. 

Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.

• increases, decreases

• increases, increases

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which of the following elements has the smallest atomic radius?

• Sulfur

• Chlorine

• Aluminum

• Sodium

Which atom has the largest atomic radius?

• Potassium (K)

• Rubidium (Rb)

• Francium (Fr)

• Cesium (Cs)

Which of the following will have a higher electronegativity than arsenic (As)?

• Carbon (C)

• Neon (Ne)

• Antimony (Sb)

• Germanium (Ge)

Tags

NGSS.HS-PS1-1

The element with the largest electronegativity in the halogens is - 

• At
• F
• Cl
• Br

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

The element with the lowest electronegativity in Period 3 is -

• Na

• Cl

• Ar

• Mg

Tags

NGSS.HS-PS1-2

As you look from left to right across a period, electronegativity

• increases

• decreases

The minimum energy required to remove an electron from the ground state of an atom

• electron configuration
• energy levels
• ionization energy
• ionic bond