Ionization energy
This term refers to the energy required to remove an electron from an atom in its gaseous state
What is ionization energy?
This term describes an atom’s ability to attract electrons in a chemical bond
What is electronegativity?
This term refers to the size of an atom, measured from the nucleus to the outermost electron shell
What is atomic radius?
This property of metals allows them to be hammered into thin sheets.
What is malleability?
This trend explains why fluorine has a smaller atomic radius than lithium.
What is the trend across a period (atomic radius decreases)?
This element in Period 2 has the highest ionization energy
What is neon (Ne)?
This element has the highest electronegativity value on the periodic table.
What is fluorine (F)?
This element in Period 3 has the largest atomic radius
What is sodium (Na)?
This group of metals is highly reactive and includes elements like sodium and potassium.
What are the alkali metals (Group 1)?
This property of elements increases as you move from bottom to top in a group and from left to right across a period.
What is electronegativity?
Ionization energy generally does this as you move from left to right across a period
What is increases?
Electronegativity generally does this as you move down a group
What is decreases?
Atomic radius generally does this as you move from left to right across a period.
What is decreases?
This transition metal is known for its resistance to corrosion and is used in jewelry.
What is gold (Au)?
This element has the lowest ionization energy in Period 4.
What is potassium (K)?
This alkali metal has the lowest ionization energy in Group 1
What is francium (Fr)?
This element in Period 3 has a higher electronegativity than magnesium but lower than chlorine
What is sulfur (S)?
This alkali metal has the largest atomic radius in Group 1.
What is francium (Fr)?
This property of metals allows them to conduct electricity and heat.
What is conductivity?
This trend explains why cesium is more reactive than sodium.
What is the trend down a group (reactivity of metals increases)?
Why does ionization energy decrease from nitrogen to oxygen?
What is the increased electron–electron repulsion in oxygen’s paired 2p orbital that destabilizes its electrons compared to nitrogen’s half-filled configuration? (what is repulsion?)
This group of elements has the lowest electronegativity values on the periodic table
What are the alkali metals (Group 1)?
This noble gas has the smallest atomic radius in Period 2.
What is helium (He)?
This metal is liquid at room temperature and is found in thermometers.
What is mercury (Hg)?
This element has the highest electron affinity in the periodic table.
What is chlorine (Cl)?