stuff

Question 1

Mendeleev

Answer 1

created the periodic table of elements

Question 2

rutherford

Answer 2

discovered the nucleus in gold foil experiment

Question 3

dalton

Answer 3

first dude to prove that all matter is made of atoms and that chemical reactions were simply rearrangements.

Question 4

thomson

Answer 4

first proposed that atoms were made up of positive and negative charges

Question 5

bohr

Answer 5

proposed that electrons in an atom don’t exist as a cloud of negative charges, but rather occupy specific “orbits” around the nucleus with specific energies associated with them. Electrons can only absorb from one “orbit” to another, so they have to be in shells

Question 6

proton, electron, and neutron size

Answer 6

p = 1 AMU 
e = almost 0
n = slightly more than 1 AMU

Question 7

atomic number

Answer 7

number of protons in the nucleus

Question 8

atomic mass

Answer 8

average m ass of all isotopes of the element = the one with the decimal

Question 9

mass number

Answer 9

atomic mass rounded to the nearest whole number OR protons plus neutrons

Question 10

ion charge (combining capacity)

Answer 10

the charge on ions of the element

Question 11

neutrons

Answer 11

atomic mass - atomic number

Question 12

quantum of energy

Answer 12

the difference in energy between two energy levels

Question 13

orbital

Answer 13

describes where electrons can be found in an atom

Question 14

s-subshell

Answer 14

sphere-shaped
contains 1 orbital
can contain 2 electrons
lowest energy subshell
exists in every shell

Question 15

p-subshell

Answer 15

peanut-shaped
contains 3 orbitals
can contain 6 electrons
exists only in the second shell and larger shells

Question 16

d-subshell

Answer 16

“double peanut” shape
contains 5 orbitals
can contain 10 electrons
only exists in third shell and larger shells
is shifted by one energy level on the periodic table (like if you see it in the 4th row then it is in the third shell)

Question 17

f-subshell

Answer 17

flower shape
contains 7 orbitals
can contain 14 electrons
exists only in the fourth shell and larger shells
is shifted by 2 energy levels on the periodic table (so if you see it in the sixth row, then it is in the fourth shell)

Question 18

valence electrons

Answer 18

all electrons outside of the core and electrons in filled d and f subshells

Question 19

laws of electrostatic forces

Answer 19

1) opposite charges attract
2) like charges repel
3) the greater the distance between the charges, the smaller the electrostatic force between them
4) the greater the charge on the particles, the greater the electrostatic force between them

Question 20

atomic number and electrostatic forces

Answer 20

as you go from left to right across a period, the atomic number increases = the number of protons in the nucleus increases = the amount of positive charges on the nucleus increases
but the average distance from the nucleus to the electron shells remain the same

Question 21

atomic radius and electrostatic forces

Answer 21

as you go from left to right across a period, the atomic radius decreases. if there’s a higher charge, it shrinks because of higher attraction. if there’s a lower charge, it expands a bit because of lower attraction
as you go from top to bottom within a group, the number of electron shells increases. therefore, the atomic radius increases because when there are more layers, its wider

Question 22

ionization energy

Answer 22

the amount of energy required to remove an electron from a neutral atom form a positive ion (K + energy = K+)
it increases as you go from left to right. the further the right, the higher the charge, thus the higher the attraction, thus the more energy is needed to pull them apart
as you go from top to bottom within a group, the ionization energy decreases because the distance between the nucleus and the electrons increase, so the attraction goes down.

Question 23

shielding effect

Answer 23

competition between attraction of nucleus and repelling of electrons

Question 24

polar molecules dissolve in ___

non-polar molecules dissolve in ___

Answer 24

polar solutions

non-polar solutions

Question 25

electronegativity

Answer 25

the tendency of an atom to attract the electrons of another atom
in general, as you go from left to right across a period, the electronegativity increases
in general, as you go from top to bottom within a group, the electronegativity decreases

Question 26

ionic bonds

Answer 26

the difference in electronegativity is greater than 1.6

Question 27

covalent bonds

Answer 27

the difference in electronegativity is less than 0.2

Question 28

polar covalent bond

Answer 28

results when the difference in electronegativity is between 0.2 and 1.6. it is a partial separation of charge = dipole

Question 29

anions

Answer 29

negatively charged ions (gained electrons)

Question 30

cations

Answer 30

positively charged ions (lost electrons)

Question 31

the greeks

Answer 31

early form of elements, earth water fire and air

Question 32

water is (polar/non-polar)
hexane is (polar/non-polar)

Answer 32

polar

non-polar

Question 33

polar molecule

Answer 33

unequal dipoles do not cancel out