chem chapter 6 quiz

Question 0

all atoms need 8 electrons, except…

Answer 0

hydrogen needs 2, boron needs 6, beryllium needs 4

Question 1

what element is usually the central atom in lewis structure

Answer 1

least electronegative

Question 2

the number of available electrons is equal to the _____________

Answer 2

number of valence electrons of the atom

Question 3

shared electrons=

Answer 3

N-A (always even)

Question 4

number of bonds=

Answer 4

S/2

Question 5

H is never involved in a multiple bond

___,____ and ___ often form double and triple bonds

Answer 5

C, N, O

Question 6

total number of electrons should equal the ______ number

Answer 6

A

Question 7

what is the metallic trend

Answer 7

increases up to down, right to left

Question 8

what is the atomic radii trend

why

Answer 8

increases up to down(valence electron is occupying higher energy level/n value increases making radius larger), increases right to left (number of protons increases (nuclear charge) pulling the electrons in tighter making the radius smaller

Question 9

the differences in electronegativities is the classifier of bonds, what are the ranges for each

Answer 9

polar covalent 1.7>or equal to x > or equal to .5
pure covalent x<.5
ionic x>1.7

Question 10

isoelectronic means?

Answer 10

same number of electrons

Question 11

what is the atomic radii

Answer 11

distance from the center of the nucleus to the “edge” of the electron cloud
usually measured in picometers or angstroms (1x10^-10m)
must be in gas form
center of nucleus to center of nucleus divided by 2

Question 12

what is the atomic radii trend for cations?

anions?

Answer 12

cations: increases up to down, right to left
anions: increases up to down, left to right

Question 13

when hydrogen becomes an ion, it is just an ____

Answer 13

electron

Question 14

______ do not have ionic radii because they do not form ions

Answer 14

noble gases

Question 15

what is shielding effect

Answer 15

inner electrons shield valence electrons from positive charge of the nucleus (protons) (concert analogy)

Question 16

what is the ionization energy trend

Answer 16

increases down to up, left to right

Question 17

ionization energy is always _____ meaning energy is added to the atom to remove the electron

Answer 17

endothermic

Question 18

how are ionization energy and atomic radius related

Answer 18

inversely proportional

Question 19

what is ionization energy

Answer 19

the energy required to move an electron from an atom is ionization energy

Question 20

the larger the atom is, the (harder/easier) it is for electrons to be removed

Answer 20

easier

Question 21

why does ionization energy increase left to right? down to up?

Answer 21

because atoms towards the right do not want to gain electrons, they want to lose
because the electrons are held in lower-energy orbitals, closer to the nucleus and therefore are more tightly bound (harder to remove).

Question 22

what is the electron affinity trend

Answer 22

increases down to up, left to right

Question 23

what is electron affinity

Answer 23

a measure of the energy change when an electron is added to a neutral atom to form a negative ion

Question 24

what is electron affinity opposite of

Answer 24

ionization energy

Question 25

why does electron affinity increase down to up, left to right

Answer 25

because the electrons added to energy levels become closer to the nucleus, thus a stronger attraction between the nucleus and its electrons

Question 26

what is the electronegativity trend

Answer 26

increases down to up, left to right

Question 27

what is electronegativity

Answer 27

holding onto its own electrons and taking other ones

Question 28

why does electronegativity increase down to up and left to right

Answer 28

This occurs due to a greater charge on the nucleus, causing the electron bonding pairs to be very attracted to atoms placed further right on the periodic table

Question 29

what is the difference between electron affinity and ionization energy

Answer 29

electron affinity is a measure of the energy change when an electron is added while ionization energy is the energy required to remove an electron

Question 30

why does fluorine have a higher ionization energy than iodine?

Answer 30

it has less electrons-lesser shielding/greater attraction between the electrons and the nucleus

Question 31

why do elements in the same family generally have similar properties

Answer 31

they have the same amount of valence electrons