Quantum Theory

Front 1

Always equal to the number of protons

Back 1

Atomic Number

Front 2

The Atomic Number equals to the number of electrons if it has no ______/ ______

Back 2

Charge/ neutral

Front 3

Proton+ Neutron =?

Back 3

Mass Number

Front 4

The number of chemical element in the periodic system

Back 4

Atomic Number

Front 5

Proton- Mass Number=?

Back 5

Neutrons

Front 6

In electrons if the charge is positive

Back 6

Subtract

Front 7

In electrons if the charge is negative

Back 7

Add

Front 8

Atoms with the same atomic numbers but different mass numbers (that is, of the same number of protons but different numbers of neutron

Back 8

ISOTOPES

Front 9

Different elements,same mass number

Back 9

ISOBARS

Front 10

Different elements , same number of neutrons

Back 10

ISOTONES

Front 11

A field of physics that is required to understand phenomena at the molecular and atomic levels

Back 11

Quantum Theory

Front 12

Set of numbers used to describe the position and energy of the electron ian atom

Back 12

Quantum Numbers

Front 13

What are the Quantum Numbers?

Back 13

Principal

Angular Momentum/Azimuthal

Magnetic

Spin

Front 14

What is the symbol of principal?

Back 14

n

Front 15

What is the symbol of Angular Momentum/Azimuthal?

Back 15

l

Front 16

What is the symbol of Magnetic?

Back 16

m/ml

Front 17

What is the symbol of spin?

Back 17

s/ms

Front 18

What is the values of principal?

Back 18

1,2,3,4

Front 19

What is the values of Angular Momentum/Azimuthal?

Back 19

0 to n-1

s=1; l=0=1=2

p=n=2; l=0,1=3=6

d=n=3; l=0,1,2,5=10

f=n=4; l=0,1,2,3=7=14

Front 20

What is the values of magnetic?

Back 20

-l to +l

Front 21

What is the values of spin?

Back 21

-1/2 or +1/2

Front 22

What is the functions of principal?

Back 22

-Size of the electron cloud

-Main energy level or shell

Front 23

What is the functions of Angular Momentum/Azimuthal?

Back 23

-shape of the electron cloud

- subshell/sublevel

Front 24

What is the functions of magnetic?

Back 24

Orientation of the space of electron cloud

Front 25

What is the functions of spin?

Back 25

Direction of the spin or rotation

Front 26

Is a region of probability surrounding the nucleus

Back 26

Shell

Front 27

What are the types of shells?

Back 27

K,L,M,N

Front 28

Is a collection of one or more orbitals of a specific type

Back 28

Subshells

Front 29

What are the types of subshells?

Back 29

S,P,D,F

Front 30

What is the meaning of the subshell s?

Back 30

Sharp

Front 31

What is the meaning of the subshell p?

Back 31

Principal

Front 32

What is the meaning of the subshell d?

Back 32

Diffuse

Front 33

What is the meaning of the subshell f?

Back 33

Fundamental

Front 34

Is a specifically shaped region of a space around the nucleus where an electron is mostly found

Back 34

Orbitals

Front 35

What is the equivalents of electrons in the orbital?

n=1 or K-shell=

n=2 or L-shell=

n=3 or M-shell=

n=4 or N-shell=

Back 35

1x2=2

2x4=8

3x6=18

4x8=32

Front 36

What are the four inorganic chemistry principle?

Back 36

Pauli's Exclusion Principle

Aufbau/ Building Up Principle

Hund's rule of maximum Multiplicity

Heisenberg Uncertainty

Front 37

INORGANIC CHEMISTRY PRINCIPLE

No two electrons can have the same set of quantum numbers

Back 37

Pauli's Exclusion Principle

Front 38

INORGANIC CHEMISTRY PRINCIPLE

Lower energy levels are paired up first

Back 38

Aufbau/ Building Up Principle

Front 39

INORGANIC CHEMISTRY PRINCIPLE

Orbitals are filled up singly before pairing up

Back 39

Hund's Rule of Maximum Multiplicity

Front 40

INORGANIC CHEMISTRY PRINCIPLE

It is impossible to determine simultaneously the momentum and position of an atom

Back 40

Heisenberg Uncertainty

Front 41

Group of numbers which shows the arrangement of the electrons in an atom

Back 41

Electron Configuration

Front 42

What is the electron configuration of Na?

Back 42

1s2 2s2 2p6 3s1

Front 43

Give the quantum number values of the element, Nitrogen

Back 43

Electron Configuration

1s2 2s2 2p3

Focus on the last of numbers of the EN

2p3

Principal Quantum Number

n=2

Azimuthal Quantum Number

l= 0,1

Magnetic Quantum Number

ml= -1,0,1

Front 44

What are the laws of chemical combination?

Back 44

Dalton's Atomic Theory

Law's of Conservation of Mass

Law of Definite Proportions

Law of Multiple Proportions

Front 45

LAW OF CHEMICAL COMBINATION

1.Each element is composed of extremely small particles called atoms.2. All atoms of the same elements are identic, and different elements have different type of atoms3. Atoms of one element cannot be changed into atoms of a different element by chemical reactions4. Compounds are formed when atoms of more than one element

Back 45

Dalton's Atomic Theory

Front 46

LAW OF CHEMICAL COMBINATION

Atoms are neither created nor destroyed

Back 46

Law of Conservation of Mass

Front 47

LAW OF CHEMICAL COMBINATION

Samples of a given compound always contain the same proportion of elements by mass

Back 47

Law of Definite Proportions

Front 48

Another term for law of definite proportions

Back 48

Proust's Law or the Law of Constant Composition

Front 49

LAW OF CHEMICAL COMBINATION

When one element combines with another to form more than one compound, the mass ratios of the elements in the compounds are simple whole number of each other.

Back 49

Law of Multiple Proportions

Front 50

Who are the proponents that are involved in the periodic table?

Back 50

Johann Dobereiner

John Newlands

Meyer and Mendeleev

Henry Moseley

Antoine Laurent Lavoisier

Front 51

Proposed the law of triads based on the physical and chemical properties of elements

Back 51

Johann Dobereiner

Front 52

How does the law of triads works?

Back 52

Wherein you add the first and the third/last element and then divide by two, you'll get the atomic mass of the second element

Front 53

Law of octaves, states that every eighth element has similar properties when it's elements are arranged in the increasing order of their atomic masses

Back 53

John Newlands

Front 54

-Physical and chemical properties are periodic function of their periodic weight

Back 54

Meyer and Mendeleev

Front 55

Grouped the element based on their properties into gases,nonmetals,metals, and earths

Back 55

Antoine Laurent Lavoisier

Front 56

A pure substance composed of a single atom with a unique atomic number

Back 56

Element

Front 57

The vertical column of the periodic table that signifies the the number of valence electron in an element

Back 57

Group

Front 58

The horizontal rows in the periodic table that signify the number of electron shells in an element

Back 58

Periods

Front 59

Elements that have the same number of valence electrons and therefore similar properties

Back 59

Families

Front 60

Considered as the Father of Modern Chemistry

Back 60

Antoine Laurent Lavoisier

Front 61

Family A (Representative Elements)

Back 61

S and P block

Front 62

Family B (Transition Elements)

Back 62

D and F block

Front 63

Identify the Elements by its last electronic configuration

Back 63

2p6-

4s2-

3p6

Front 64

One half the distance between the nuclei of two adjacent atoms

Back 64

Atomic Radius/Atomic Size

Front 65

Atomic radius increases from _______ and ______

Back 65

Right to Left

Top to Bottom

Front 66

The level of reactivity of a metal when it loses an electron in a chemical reaction

Back 66

Metallic Property

Front 67

Metallic property increases from _______ and ____

Back 67

right to left

top to bottom

Front 68

Tendency of an atom to attract electrons

Back 68

Electronegativity

Front 69

Ability of an atom to remove electron from an atom

Back 69

Ionization Energy

Front 70

Ionization energy increases from____ and _______

Back 70

left to right

bottom to top

Front 71

Ability of an atom to accept an electron from an atom

Back 71

Electron Affinity

Front 72

Electron affinity increases from ______ to _______ and _____ to ______.

Back 72

Left to right

Bottom to top

Front 73

During chemical changes, atoms can lose or gain electrons and become charged particles

Back 73

Ions

Front 74

Positively charged ions;produced when an atom loses an electron

Back 74

Cations

Front 75

Negatively charged ions; produced when an atom gains an electron

Back 75

Anions

Front 76

An ion that contains more than one atom

Back 76

Polyatomic Ions

Front 77

Chalk

Back 77

Calcium Carbonate

Front 78

Charge of Beam

Cathode-

Anode-

Back 78

Cathode (-)

Anode (+)

Front 79

Arranged the elements in the periodic table according to atomic numbers

Back 79

Henry Moseley

Front 80

What is the shape s-orbital?

Back 80

Sphere

Front 81

What is the shape p-orbital?

Back 81

Dumbbell

Front 82

What is the shape d-orbital?

Back 82

Clover

Front 83

What is the shape f-orbital?

Back 83

Hybrid