Periodic Table, Atoms, Ions, & Molecules

Question 1

Who created the Planetary Model of an atom?

Answer 1

Niel’s Bohr

Question 2

What is J.J. Thomson’s atomic model?

Answer 2

Plum pudding model

Question 3

He created the Electron Cloud/Quantum Model of an atom

Answer 3

Erwin Schrodinger

Question 4

He created the Solid Sphere Model otherwise known as the Billiard Ball Model

Answer 4

John Dalton

Question 5

What is Ernest Rutherford’s proposed atomic model?

Answer 5

Nuclear Model

Question 6

Define orbital

Answer 6

It is a region in space where the probability of finding an electron is the highest; It is where you could find electrons moving around/orbiting the nucleus at a lightning pace

Question 7

It is the function developed by Erwin Schrodinger in his cloud model to describe a cloud-like region where the electron is likely to be found

Answer 7

The probability function

Question 8

How many electrons can be accommodated in each orbital?

Answer 8

s-orbital: 2
p-orbital: 6
d-orbital: 10
f-orbital: 14

Question 9

Describe the relationship between the electron configuration and the periodic table

Answer 9

By looking at the electron configuration of an element, specifically at its last electron, we will be able to locate the position of that element in the periodic table.

For example, the last electron of carbon is 2p^2. Therefore, it is located on the second period (based on the coefficient of p), on the second column (based on the superscript of p) of the p-block on the right side of the table.

Question 10

It also represents the number of electron shells of the element

Answer 10

Period

Question 11

TRUE or FALSE: Only the representative elements (from Group 1A-8A) have their group numbers also correspond to the number of their valence electrons

Answer 11

TRUE

Question 12

It states that electrons fill lower-energy atomic orbitals before filling higher-energy ones

Answer 12

Aufbau (building-up) Principle

Question 13

According to this rule electron pairing in p, d and f orbitals cannot occur until each orbital of a given subshell contains one electron each or is singly occupied.

Answer 13

Hund’s Rule (of Maximum Multiplicity)

Question 14

It states that no two electrons can have the same set of 4 quantum numbers

Answer 14

Pauli Exclusion Principle

Question 15

This quantum number tells you the period number / energy level or shell where an atomic orbital can be found.

Answer 15

Principal quantum number

Question 16

It also describes how far away from the nucleus the shell or energy level under consideration is. The lower the number, the closer the energy level is to the atom’s nucleus.

Answer 16

Principal quantum number

Question 17

It represents the shape or the kind of sublevel or orbital (spdf) that is being occupied by the electron

Answer 17

Secondary quantum number/Azimuthal quantum number/Angular quantum number

Question 18

What are the symbols of the four quantum numbers?

Answer 18

(n, l, ml ms)

Question 19

Enumerate the angular quantum number of each orbital type

Answer 19

s: l = 0
p: l = 1
d: l = 2
f: l = 3

Question 20

How do we determine the secondary quantum number?

Answer 20

l = n-1

Question 21

It indicates the kind of suborbital within the sublevel where the electron is found.

Answer 21

Magnetic quantum number

Question 22

What are the possible values of magnetic quantum numbers for each angular quantum number/sublevel?

Answer 22

0 - 0
1 - -1, 0, +1
2 - -2, -1, 0, +1, +2
3 - -3, -2, -1, 0, +1, +2, +3

Question 23

Describes the direction (clockwise or counter-clockwise) in which an electron spins

Answer 23

Spin quantum number

Question 24

Why are +- 1/2 the only possible values for the spin quantum number

Answer 24

Two electrons in one suborbital are given 50% each

Question 25

Describe the properties of an electron associated with each of the following four quantum numbers: n, l, ml, and ms

Answer 25

n - energy level or how far an electron is from the nucleus (The lower the number, the closer the energy level is to the atom's nucleus; the closer the electron is to the nucleus, the lower its energy) l - shape of the orbital (s, p, d, f) ml - orientation of the orbital with respect to the same l value (i.e. positive or negative) ms - spin of the electron

Question 26

What are the atomic properties with periodic trends?

Answer 26

atomic size (radius), ionization energy, electron affinity, electronegativity

Question 27

Describe the Rules on Filling of Atomic Orbitals

Answer 27

1. Aufbau Principle - 2. Hund's Rule of Multiplicity - 3. Pauli Exclusion Principle -

Question 28

It represents the distance of the boundary surrounding the cloud of electrons to the nucleus

Answer 28

Atomic size

Question 29

It is the number of protons in the nucleus of an atom

Answer 29

Atomic number

Question 30

It refers to the number of protons and neutrons in an atom

Answer 30

Mass number

Question 31

It describes the tendency of an atom to attract electrons towards itself

Answer 31

Electronegativity

Question 32

It is the amount of energy required to remove an electron from an atom/molecule to form a positive ion

Answer 32

Ionization energy

Question 33

It is the amount of energy released when an electron is added to a neutral atom/molecule to form a negative ion

Answer 33

Electron affinity

Question 34

What are the atomic radius trends?

Answer 34

LEFT TO RIGHT (ACROSS A PERIOD) - DECREASES TOP TO BOTTOM (GOING DOWN A GROUP) – INCREASES

Question 35

Why does the atomic size decrease from left to right within a period?

Answer 35

Because as more electrons are being added to the same shell, more protons are also being added to the nucleus, making it more positively charged. In turn, the nucleus is able to attract more outer electrons and pulls their shells closer to its center More protons, more effective nuclear charge, and therefore smaller atomic size

Question 36

What is the periodic trend for ionization energy?

Answer 36

LEFT TO RIGHT (ACROSS A PERIOD) - INCREASES TOP TO BOTTOM (GOING DOWN A GROUP) - DECREASES

Question 37

What are the trends for electron affinity?

Answer 37

LEFT TO RIGHT (ACROSS A PERIOD) - INCREASES TOP TO BOTTOM (GOING DOWN A GROUP) - DECREASES

Question 38

What are the trends for electronegativity?

Answer 38

LEFT TO RIGHT (ACROSS A PERIOD UNTIL GROUP 7A) - INCREASES TOP TO BOTTOM (GOING DOWN A GROUP) - DECREASES

Question 39

Which is more electronegative? metals or non-metals?

Answer 39

Non-metals

Question 40

What are the 4 natures of matter according to Dalton's atomic theory?

Answer 40

1. Elements are composed of extremely small particles called atoms. 2. All atoms of a given element are identical, having the same size, mass, and chemical properties. The atoms of one element are different from the atoms of all other elements. 3. Compounds are composed of atoms of more than one element. For any given compound, the atoms present are always in the same ratio. 4. A chemical reaction involves only the separation, combination, or rearrangement of atoms; it does not result in the creation or destruction of atoms

Question 41

According to the law, if two elements can combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element are in ratios of small whole numbers

Answer 41

Law of multiple proportions

Question 42

It states that different samples of the same compound always contain its constituent elements in the same proportions by mass

Answer 42

Law of definite proportions

Question 43

TRUE or FALSE: Neutrons are present in the nucleus of all atoms except hydrogen

Answer 43

TRUE

Question 44

Atomic number (Z) vs Mass number (A)

Answer 44

Z - # of protons A - protons + neutrons / Z + neutrons

Question 45

Protons and neutrons in the nucleus are collectively known as?

Answer 45

Nucleons

Question 46

These are atoms that have the same Z but different A

Answer 46

Isotopes

Question 47

He discovered neutrons

Answer 47

James Chadwick

Question 48

What was the experiment conducted by Robert Millikan that led to the discovery of the charge of an electron?

Answer 48

Oil drop experiment

Question 49

Who discovered the electron?

Answer 49

JJ Thomson

Question 50

He did the gold foil experiment that led to the discovery of protons

Answer 50

Ernest Rutherford

Question 50

He did the gold foil experiment that led to the discovery of protons

Answer 50

Ernest Rutherford

Question 51

It refers to an atom with a net positive or negative charge

Answer 51

Ion

Question 52

Atoms that have the same number of protons but different number of neutrons

Answer 52

Isotopes

Question 53

One of two or more distinct forms of an element

Answer 53

Allotrope

Question 54

Good conductors of heat and electricity

Answer 54

Metals

Question 55

Poor conductors of heat and electricity

Answer 55

Non-metals