Unit 10 test

Question 1

ionization energy trends

Answer 1

decrease from top to bottom, increase from left to right

Question 2

electronegativity trends

Answer 2

decrease from top to bottom, increase from left to right

Question 2

ionization energy definition

Answer 2

energy required to move an electron from an atom in its gaseous state

Question 2

electronegativity definition

Answer 2

the ability of a gaseous atom to attract electrons

Question 3

electron affinity trends

Answer 3

decrease from top to bottom, increase from left to right

Question 4

electron affinity definition

Answer 4

change in energy of a neutral gaseous atom when an electron is added to the atom

Question 4

atomic size/ radii trends

Answer 4

increases from top to bottom, decreases from left to right

Question 5

atomic size/ radii definition

Answer 5

1/2 the distance between the nuclei of 2 adjacent atoms of the same element when the atoms are joined

Question 6

ionic size/ radii definition

Answer 6

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

Question 7

ionic size/ radii trends

Answer 7

increases from top to bottom, decreases from left to right

Question 8

energy trend

Answer 8

decrease from top to bottom, increase from left to right

Question 9

size/ radii trend

Answer 9

increases from top to bottom, decreases from left to right

Question 10

ionic bonds

Answer 10

electrostatic attraction between cation and anion

Question 10

covalent bonds

Answer 10

sharing of valence electrons

Question 11

meaning of polar or polar covalent bonds

Answer 11

there is an uneven sharing of valence electrons; one atom is more negative and the other atom is less negative

Question 12

difference between polar covalent and no polar covalent bonds

Answer 12

non polar is the even sharing of valence electrons; the more polar the bond the more the bond behaves like an ionic bond

Question 13

how do electronegativity values help us determine the type of bond created

Answer 13

if we have the electronegativity values for the 2 bonded atoms, we can find the difference in electronegativity values

Question 14

non polar bond range

Answer 14

0-0.4

Question 14

slightly polar bond range

Answer 14

0.5-0.9

Question 15

ionic bond range

Answer 15

1.8+

Question 15

very polar bond range

Answer 15

1.0-1.7

Question 15

ionic bonding properties

Answer 15

• 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

Question 16

metallic bonding properties

Answer 16

• 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

Question 17

covalent bonding properties

Answer 17

• 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

Question 18

horizontal row on the periodic table

Answer 18

period

Question 19

electrons

Answer 19

subatomic particles that are transfered to form positive and negative ions

Question 19

vertical column in the periodic table

Answer 19

group