Unit 10 test Flashcards
ionization energy trends
decrease from top to bottom, increase from left to right
electronegativity trends
decrease from top to bottom, increase from left to right
ionization energy definition
energy required to move an electron from an atom in its gaseous state
electronegativity definition
the ability of a gaseous atom to attract electrons
electron affinity trends
decrease from top to bottom, increase from left to right
electron affinity definition
change in energy of a neutral gaseous atom when an electron is added to the atom
atomic size/ radii trends
increases from top to bottom, decreases from left to right
atomic size/ radii definition
1/2 the distance between the nuclei of 2 adjacent atoms of the same element when the atoms are joined
ionic size/ radii definition
the distance between the nuclei of a cation and an adjacent anion in an atomic radius, the radius of a cation or anion, or both
- cations are always SMALLER than the parent atom
-anions are always LARGER than the parent atom
ionic size/ radii trends
increases from top to bottom, decreases from left to right
energy trend
decrease from top to bottom, increase from left to right
size/ radii trend
increases from top to bottom, decreases from left to right
ionic bonds
electrostatic attraction between cation and anion
covalent bonds
sharing of valence electrons
meaning of polar or polar covalent bonds
there is an uneven sharing of valence electrons; one atom is more negative and the other atom is less negative
difference between polar covalent and no polar covalent bonds
non polar is the even sharing of valence electrons; the more polar the bond the more the bond behaves like an ionic bond
how do electronegativity values help us determine the type of bond created
if we have the electronegativity values for the 2 bonded atoms, we can find the difference in electronegativity values
non polar bond range
0-0.4
slightly polar bond range
0.5-0.9
ionic bond range
1.8+
very polar bond range
1.0-1.7
ionic bonding properties
- metal + nonmetal
-atoms seek stability
-atoms give off or receive electrons
-happens between atoms with great differences in electronegativity
-easily breaks
-ability to conduct may depend on state - high melting and boiling point
metallic bonding properties
- metal + metal
-atoms seek stability
-atoms release electrons to become cations
-can bend without breaking
-can conduct heat and electricity
-high melting and boiling point
covalent bonding properties
- nonmetal + nonmetal
- atoms seek stability
-atoms share electrons with other atoms
-happens between atoms with little difference in electronegativity
-fragility depends on state
-ability to conduct may depend on the atoms
-low melting and boiling point
horizontal row on the periodic table
period
electrons
subatomic particles that are transfered to form positive and negative ions
vertical column in the periodic table
group
