Chapter 1

Question 1

What is all matter composed of?

Answer 1

atoms which are subatomic particles

Question 2

protons carry what charge and have what mass?

Answer 2

+1 charge and have a mass of 1 amu/ 1 Da actual charge is 1.6 x 10^-19 C

Question 3

Neutrons have what charge and what mass

Answer 3

neutral and 1 amu

Question 4

protons and neutrons can be called what?

Answer 4

nucleons

Question 5

electrons have what charge and mass

Answer 5

-1 charge and negligible mass actual charge is -1.6 x 10^-19 C

Question 6

What is the atomic number (Z)

Answer 6

the number of protons of the atom and gives the element its unique identity

Question 7

What is the mass number (A)

Answer 7

the total number of neutrons and protons contained in the nucleus

Question 8

what is an isotope

Answer 8

atoms of the same element that have different numbers of neutrons

Question 9

What is Deuterium (D or 2H)

Answer 9

An isotope of (1H that has no neutrons) that has one proton and one neutron

Question 10

what is a cation

Answer 10

ions that carry a net positive charge

Question 11

what is an anion

Answer 11

ions that carry a net negative charge

Question 12

polyatomic ions that have positive charges

Answer 12

• represented by roman numerals - the ion with lesser charge uses suffix -ous - the ion with greater charge use suffix -ic

Question 13

polyatomic ions with oxygen

Answer 13

• use suffix -ite for fewer oxygens - use suffix -ate for more oxygen atoms

Question 14

polyatomic ions with hydrogen

Answer 14

• one hydrogen is hydrogen (atom name) - two hydrogens is dihydrogen (atom name)

Question 15

Bohr model of the hydrogen atom:

Answer 15

electrons orbit the nucleus in spherical shells

Question 16

Electrons closest to the nucleus…

Answer 16

experience the greatest attractive force so it has greater stability and lower energy level

Question 17

electrons furthest from the nucleus…

Answer 17

have a higher energy level and be less stable

Question 18

what is the ground state

Answer 18

the lowest possible energy level closest to the nucleus

Question 19

when is an electron excited

Answer 19

when it absorbs energy equal to the difference between a higher shell’s energy level and the ground states energy level and jumps to the higher-energy shell

Question 20

when an electron jumps back down to ground state?

Answer 20

energy is emitted in the form of a photon

Question 21

energy is admitted and absorbed in the form of

Answer 21

electromagnetic radiation

Question 22

the energy of electromagnetic radiation formula is

Answer 22

E=hf (h = Plank’s constant 6.63 x 10^-34 J) (f = frequency of light)

Question 23

E=hf can also be described as…

Answer 23

E = hc/ wavelength (h = Plank’s constant 6.63 x 10^-34 J) (c = speed of light 3.00 x 10⁸ m/s is a vacuum)

Question 24

equation to calculate the energy level held by an electron at a certain energy level

Answer 24

E = -(R/n²) R = Rydberg constant 2.18 x10^-18 J) n = energy level at which the electron is present

Question 25

Rydberg formula determines the energy level and wavelength of the emitted or absorbed radiation as an electron moves

Answer 25

deltaE=hc/wavelength= R(1/nf² - 1/ni²) R = Rydberg constant 2.18 x10-18 J) n = energy level at which the electron is present

Question 26

Moving from a higher to a lower energy level is associated with

Answer 26

emission

Question 27

moving from a lower level to a higher one

Answer 27

requires energy absorption

Question 28

Heisenberg uncertainty principle

Answer 28

posits that the more we know about the position of an electron, the less we know about its momentum and vice versa (cannot know both position and momentum of an electron at the same time)

Question 29

system of quantum numbers

Answer 29

helps describe electrons to an extent

Question 30

electrons exist in?

Answer 30

orbitals (areas of space where electrons are likely to be located)

Question 31

each orbital can hold how many electrons

Answer 31

max of 2

Question 32

principal quantum number (n)

Answer 32

the energy level of the electron (1 or greater) - relates to the row of the table in which the element is found

Question 33

azimuthal or angular momentum quantum number (l)

Answer 33

describes the sub shell of the principal quantum number where the electron is found and range from 0 to n - 1 l = 0 is the s subshell l = 1 is the p subshell l = 2 is the d subshell l = 3 is the f subshell

Question 34

magnetic quantum number (ml)

Answer 34

describes the spatial orientation of the orbital in question within its subshell l = 0 holds one orbital l = 1 holds 3 orbitals l = 2 holds 5 orbitals l = 3 holds 7 orbitals

Question 35

spin quantum number (ms)

Answer 35

describes the spin orientation of the electron which relates to its angular momentum -1/2 or +1/2 2 electrons in same orbital have opposite spin

Question 36

electron configuration

Answer 36

describes the arrangement of electrons in sub shells around the atomic nucleus ex. A 3d subshell that contains 8 electrons would be denoted as 3d⁸

Question 37

Aufbau principle

Answer 37

electrons fill lower-energy orbitals first to create the most stable electron configuration

Question 38

Hund's rule

Answer 38

each electron would rather exist in an orbital by itself if possible so we fill each half way first then fill

Question 39

Element blocks of the periodic table

Answer 39

Question 40

valence electrons are

Answer 40

the electrons furthest away from the nucleus

Question 41

periods are also known as columns are also known as

Answer 41

1. rows 2. families

Question 42

division of the periodic table

Answer 42

Question 43

effective nuclear charge (Z_eff)

Answer 43

the attractive force of the nucleus on the atom's valence electrons as number of protons increases from left to right, Z_eff also increases but moving down the table Z_eff decreases

Question 44

atomic size or radius

Answer 44

inversely related to Z_eff so as we go from left to right, atomic size decreases but as we go down, it increases

Question 45

ionic radius (the radius of a charged speices)

Answer 45

ionic radius of a cation is smaller than the ionic radisu of an anion in comparison to an uncharged form

Question 46

ionization energy

Answer 46

the energy required to move one valence electron from a neutral atom in a gaseous state positive value the first ionization energy is always smaller than the second directly related to Z_eff so it increases from left to right and decreases as we go down columns

Question 47

electron affinity

Answer 47

denotes the amount of energy released when an electron is added to an atom atoms that can more readily accept an electron, such as holegns have higher electron affinities. Directly related to Z_eff so increases from L to R and decreases from up to down exception is noble gases because they posess stable octet

Question 48

electronegativity

Answer 48

the tendency of an atom to attract electrons that are shared in a chemical bond between 2 atoms direclty related to Z_eff, increases from L to R and decreases from up to down

Question 49

difference between electron affinity and electronegativity

Answer 49

electronegativity direclty relates to behaviour within a chemical bond

Question 50

trends summarized

Answer 50

all related to Z_eff except atomic size/radius