Periodicity

What makes a valence electron more attracted to the nucleus?

• less distance between the nucleus and having less protons

• less distance between the nucleus and having more protons

• more distance between the nucleus and having less protons

• more distance between the nucleus and having more protons

• less distance and having more valence electrons

Tags

NGSS.HS-PS1-1

Why doesn't having more protons increase the attraction down a column?

• there are more valence electrons in the outermost shell

• actually, there aren't more protons in the nucleus down the column

• as shells are added, non-valence electrons block the extra protons from attracting electrons

• more neutrons block the extra protons

Tags

NGSS.HS-PS1-3

NGSS.HS-PS2-4

Periodicity is

• the recurring nature of the properties of some of the elements in the periodic table

• the recurring nature of the properties of elements in the periodic table with increasing mass

• the recurring nature of the properties of elements in the periodic table with increasing atomic number

• the recurring properties of isotopes in elements

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which statement is correct

• Ionisation energy decreases down the group because valence electrons experience strong attractive forces towards the nucleus

• Ionisation energy increases down the group because valence electrons experience weak attractive forces towards the nucleus

• Ionisation energy decreases down the group because valence electrons experience weak attractive forces towards the nucleus

• Ionisation energy increases down the group because valence electrons experience strong attractive forces towards the nucleus

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

What trend is shown here

• atomic radius increasing down group 7

• atomic radius decreasing across a period

• atomic radius increasing across a period

• atomic radius decreasing down group 7

Ionic radius is a radius of an ion. It has the same trend in metals. Considering that, ionic radius in group 1 will ................ down the group.

Radius of a Selenium (Se) atom is ........ than that of an Arsenic (As) atom.

Tags

NGSS.HS-PS1-1

Bromine (Br) is bigger than Chlorine (Cl). Iodine (I) is ............ than Chlorine (Cl).

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Electronegativity ............. from left to right in a period

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Electronegativity ................. in groups from top to bottom (down the group)