ATOMIC STRUCTURE

Question 1

Atom came from the Greek word ___ meaning “uncut” or “indivisible”

Answer 1

atomos

Question 2

A particle of matter that uniquely defines a chemical element.

Answer 2

Atom

Question 3

Mention the years (6) on the evolution of atomic theory.

Answer 3

5th century BC- 1803-1897-1911-1913-1926

Question 4

Mention the six models with their creators on the evolution of atomic theory in order.

Answer 4

Atomism (Democritus)
Solid Sphere Model (John Dalton)
Plum Pudding Model (J.J. Thomson)
Nuclear Model (Ernest Rutherford)
Planetary Model (Niels Bohr)
Quantum Model (Erwin Schrodinger)

Question 5

He stated that it is impossible to pinpoint or determine accurately both momentum and position of electron simultaneously. Who said it and what is this principle?

Answer 5

Weiner Heisenberg (UNCERTAINTY PRINCIPLE)

Question 6

Involves the small nucleus and the three elementary particles called the protons, electrons, and neutrons.

Answer 6

Modern Atomic Theory

Question 7

contains the protons and the neutrons surrounded by an electron cloud.

Answer 7

Nucleus

Question 8

___ discovered the electron using the ___ and he named his model the PLUM PUDDING MODEL

Answer 8

Joseph Jon Thomson - cathode ray tube

Question 9

Discovered protons using the CANAL RAY TUBE

Answer 9

Eugen Goldstein

Question 10

studied the alpha particles in ___, which lead to the discovery of neutron

Answer 10

Sir James Chadwick- beryllium

Question 11

____ perceived the atom as a miniature solar system and used the ____ leading to the discovery of the nucleus

Answer 11

Ernest Rutherford - alpha scattering apparatus

Question 12

+2, stopped by a thin sheet of paper

Answer 12

Alpha (Rutherford’s Experiment)

Question 13

-1, stopped by a 1 cm thick of aluminum foil

No charge, stopped by lead (neutron)

Answer 13

Beta

Question 14

What is the specific electrical charge of electron (-1)?

Answer 14

-1.602 x 10^-19

Question 15

What is the specific electrical charge of proton (+1)?

Answer 15

+ 1.602 x 10^-19

Question 16

What is the electrical charge of neutron?

Answer 16

0

Question 17

What is another term for Mass number?

Answer 17

Massenzahl

Question 18

What is another term for Atomic number?

Answer 18

Atomzahl

Question 19

What are the 4 ways to separate isotopes? (TCEF)

Answer 19

Thermal Diffusion, Centrifugation, Electrolysis, Fractional Distillation

Question 20

• Are artificial radioactive isotopes
• Are prepared by the bombardment of naturally occurring at

Answer 20

Radioisotopes

Question 21

Who discovered radioisotopes?

Answer 21

Irene and Frederic Joliot Curie

Question 22

Name of the protons and neutrons inside the nucleus

Answer 22

Nucleons

Question 23

Electrically charged atoms (positive and negative ions)

Answer 23

Ions

Question 24

Atoms having different atomic weights or mass but of the same atomic number

Answer 24

Isotopes

Question 25

Who discovered isotopes

Answer 25

Frederick Soddy

Question 26

Orderly distribution of electrons among the orbitals of an atom

Answer 26

Electron Configuration

Question 27

What do you call the s,p,d,f (2,6,10,14) format?

Answer 27

Mnemonic device

Question 28

Lowest, most stable energy state of the atom

Answer 28

Ground State

Question 29

Electrons are added one at a time to the lowest energy orbitals

Answer 29

Aufbau principle

Question 30

Aufbau principle came from the German word "___" meaning "TO BUILD UP"

Answer 30

aufbaue

Question 31

No two electrons can occupy the same quantum state simultaneously in an atom a. An orbital can hold a maximum of 2 electrons b. The electrons can occupy the same orbital if they spin in opposite direction  clockwise (upward arrow)  counterclockwise (downward arrow)

Answer 31

Pauli Exclusion Principle

Question 32

* When electrons occupy orbitals of equal energy, one electron enters each orbital until all the orbitals contain one electron with parallel spins * Second electrons then add to each orbital pairing the spins of the first electrons

Answer 32

Hund's Rule

Question 33

*Electrons in the outermost energy level *Determines the chemical properties of elements

Answer 33

Valence Electron

Question 34

Who invented Lewis Dot Structure?

Answer 34

Gilbert Lewis

Question 35

What is the NOBLE GAS CONFIGURATION of the Lewis Dot Structure?

Answer 35

Duet Rule and the Octet Rule

Question 36

Consists of the element’s symbol surrounding dots to represent the number of valence electrons

Answer 36

Lewis Dot Structure

Question 37

What are the 4 Types of Bonding?

Answer 37

1. Ionic Bonding 2. Covalent Bonding 3. Metallic Bonding 4. Intermolecular Forces of Attraction

Question 38

* Transferring of electrons * Metal donates the electron to a non-metal * Metal + non-metal * Properties of Ionic Compounds o Are solid with high melting point ( › 400°C) o Conduct electricity when in aqueous solution or in molten state

Answer 38

IONIC BONDING

Question 39

Ionic Bonding are soluble in ___.

Answer 39

polar solvents

Question 40

* Sharing of electrons * Non-metal + non-metal o Single bond (H2O, CH4) o Double bond (O2, CO2) o Triple bond (N2)

Answer 40

Covalent Bonding

Question 41

Properties of Covalent Bonding

Answer 41

1. SLG with low melting points 2. Soluble in non-polar solvents

Question 42

*Is the force of attraction that holds metals together *Consists of the attraction of the free-floating valence electrons for the positively charged metal ions *Explains many physical properties of metals

Answer 42

Metallic Bonding

Question 43

*Are the forces of attractions that exist between molecules in a compound *Cause the compound to exist in solid, liquid, or gas; and affect the melting and boiling points of compounds as well as the solubility of one substance in another

Answer 43

Intermolecular Forces of Attraction

Question 44

What is another term of Intermolecular Forces of Attraction?

Answer 44

Van der Waals forces (Johannes van der Waals)

Question 45

What are types of Intermolecular Forces of Attraction?

Answer 45

1. Dispersion forces 2. Dipole to Dipole interaction 3. Hydrogen Bond

Question 46

* Weakest of all molecular interactions among non-polar molecules (H2, Cl2) * The more electrons that are present in the molecule, the stronger the dispersion forces

Answer 46

Dispersion forces

Question 47

* Occurs between polar molecules * The partial positive charge on one molecule is electrostatically attracted to the partial negative charge on a neighboring molecule

Answer 47

Dipole to Dipole interaction

Question 48

* Are the strongest of the intermolecular forces * Important in determining the properties of water and biological molecules like protein * Occur between molecules from hydrogen being covalently bonded to either fluorine, oxygen or nitrogen

Answer 48

Hydrogen Bond