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Atoms And Molecules _LS_1

Total questions: 162

Worksheet time: 15hrs 42mins

Name
Class
Date
1.

International Union of Pure and Applied Chemistry is the full form of

(a)  

2.

Name the scientist who gave law of conservation of mass.

a)
Antoine Lavoisier
b)
Albert Einstein
c)
Marie Curie
d)
Isaac Newton
3.

Write the full form of IUPAC.

a)
Institute of Universal Physics and Chemistry
b)
International Union of Practical and Applied Chemistry
c)
International Union of Pure and Applied Chemistry
d)
Institute for Understanding Pure and Applied Chemistry
4.

Building blocks of all matter are (a)  

5.

Name the scientist who gave law of constant proportions.

a)
Albert Einstein
b)
Marie Curie
c)
Isaac Newton
d)
Joseph Proust
6.

What does the symbol ‘u’ represent?

(a)  

7.

A change in the physical state can be brought about

a)

(a) only when energy is given to the system

b)

(b) only when energy is taken out from the system

c)

(c) when energy is either given to, or taken out from the system

d)

(d) without any energy change

8.

Name the scientist who gave the atomic theory of matter.

a)
Albert Einstein
b)
Marie Curie
c)
John Dalton
d)
Isaac Newton
9.

Which postulate of Dalton’s atomic theory is the result of the law of conservation of mass given by Lavoisier?

a)
Atoms can be created in a chemical reaction
b)
Atoms can be destroyed in a chemical reaction
c)
Atoms can change into different elements in a chemical reaction
d)
Atoms cannot be created or destroyed in a chemical reaction
10.

Which aspect of Dalton's atomic theory was influenced by the Law of Constant Proportions proposed by Proust?

a)

A) The law of multiple proportions

b)

B) The law of definite proportions

c)

C) The existence of atoms as indivisible particles

d)

D) The concept of isotopes

11.

Which ancient Indian philosopher proposed the idea that all matter is composed of very small particles, and what name did he give to these particles?

a)

A) Chanakya - Paramanus

b)

B) Aryabhata - Anuvrittis

c)

C) Charaka - Doshas

d)

D) Kanada - Parmanus

12.

Name any two laws of chemical combination.

a)
Law of Gravity, Law of Inertia
b)
Law of Thermodynamics, Law of Motion
c)
Law of Reflection, Law of Refraction
d)
Law of Conservation of Mass, Law of Definite Proportions
13.

How is the size of an atom indicated?

a)
Atomic radius
b)
Atomic weight
c)
Atomic mass
d)
Atomic volume
14.

Name the unit in which the radius of an atom is usually expressed.

a)
centimeters
b)
meters
c)
kilometers
d)
picometers
e)

nanometres

15.

Write the relation between the nanometer and meter.

a)
1 nm = 0.000000001 m
b)
1 nm = 0.001 m
c)
1 nm = 0.0001 m
d)
1 nm = 1000 m
16.

The number of atoms constituting a molecule is known as its (a)  

17.

Chemical symbol of sodium is Na. What is its Latin name?

(a)  

18.
H is the chemical symbol for which element?
a)
Helium
b)
Hydrogen
c)
Mercury
19.
Na is the chemical symbol for which element? 
a)
Sodium
b)
Nitrogen
c)
Neon
20.
K is the chemical symbol for which element? 
a)
Krypton
b)
Potassium
c)
Knox
21.
Ca is the chemical symbol for which element? 
a)
Carbon
b)
Chlorine
c)
Calcium
22.
Fe is the chemical symbol for which element? 
a)
Freon
b)
Iron
c)
Flourine
23.
C is the chemical symbol for which element? 
a)
Calcium
b)
Chlorine
c)
Carbon
24.
N is the chemical symbol for which element? 
a)
Sodium
b)
Nitrogen
c)
Nickel
25.
O is the chemical symbol for which element? 
a)
Osmium
b)
Odell
c)
Oxygen
26.
Si is the chemical symbol for which element? 
a)
Silicon
b)
Sodium
c)
Sulfur
27.
He is the chemical symbol for which element? 
a)
Heehaw
b)
Helfion
c)
Helium
28.
The chemical symbol for hydrogen is
a)
Hy
b)
He
c)
H
29.
The chemical symbol for sodium is
a)
S
b)
So
c)
Na
30.
The chemical symbol for potassium is
a)
Po
b)
K
c)
Ko
31.
The chemical symbol for iron is
a)
I
b)
Fi
c)
Fe
32.
The chemical symbol for carbon is
a)
C
b)
Ca
c)
Na
33.
The chemical symbol for nitrogen is
a)
N
b)
Ni
c)
Na
34.
The chemical symbol for oxygen is
a)
Ox
b)
Pa
c)
O
35.
The chemical symbol for silicon is
a)
S
b)
Sa
c)
Si
36.
The chemical symbol for helium is
a)
H
b)
He
c)
Ha
37.
H is the chemical symbol for which element?
a)
Helium
b)
Hydrogen
c)
Mercury
38.

The chemical symbol for calcium is

a)

C

b)

Ca

c)

Na

39.
Na is the chemical symbol for which element? 
a)
Sodium
b)
Nitrogen
c)
Neon
40.
K is the chemical symbol for which element? 
a)
Krypton
b)
Potassium
c)
Knox
41.
Ca is the chemical symbol for which element? 
a)
Carbon
b)
Chlorine
c)
Calcium
42.
Fe is the chemical symbol for which element? 
a)
Freon
b)
Iron
c)
Flourine
43.
C is the chemical symbol for which element? 
a)
Calcium
b)
Chlorine
c)
Carbon
44.
N is the chemical symbol for which element? 
a)
Sodium
b)
Nitrogen
c)
Nickel
45.
O is the chemical symbol for which element? 
a)
Osmium
b)
Odell
c)
Oxygen
46.
Si is the chemical symbol for which element? 
a)
Silicon
b)
Sodium
c)
Sulfur
47.
He is the chemical symbol for which element? 
a)
Heehaw
b)
Helfion
c)
Helium
48.
The chemical symbol for hydrogen is
a)
Hy
b)
He
c)
H
49.
The chemical symbol for sodium is
a)
S
b)
So
c)
Na
50.
The chemical symbol for potassium is
a)
Po
b)
K
c)
Ko
51.
The chemical symbol for iron is
a)
I
b)
Fi
c)
Fe
52.
The chemical symbol for carbon is
a)
C
b)
Ca
c)
Na
53.
The chemical symbol for nitrogen is
a)
N
b)
Ni
c)
Na
54.
The chemical symbol for oxygen is
a)
Ox
b)
Pa
c)
O
55.
The chemical symbol for silicon is
a)
S
b)
Sa
c)
Si
56.
The chemical symbol for helium is
a)
H
b)
He
c)
Ha
57.
H is the chemical symbol for which element?
a)
Helium
b)
Hydrogen
c)
Mercury
58.

The chemical symbol for calcium is

a)

C

b)

Ca

c)

Na

59.

All matter consists of particles called

a)

Units

b)

Atoms

c)

Cubes

d)

Pints

60.

Atoms consist of parts called protons, neutrons, and

a)

Electons

b)

Haptons

c)

Neptons

d)

Wontons

61.

Each protons has a _______________ electrical charge

a)

Positive

b)

Negative

c)

Neutral

d)

Shocking

62.

Each electron has a _________________ electrical charge

a)

Positive

b)

Negative

c)

Neutral

d)

Shocking

63.

Each neutron has an electrically_________________charge

a)

Positive

b)

Negative

c)

Neutral

d)

Shocking

64.

The nucleus of an atom contains protons and_______________

a)

Electrons

b)

Haptons

c)

Neutrons

d)

Wontons

65.

Electrons move around_________________the nucleus

a)

Inside

b)

Outside

c)

On top of

d)

Without

66.

An element is determined by the number of ___________________ (also known as its atomic number).

a)

Neutrons

b)

Electrons

c)

Protons

d)

Wontons

67.

The modern periodic table is organized by _________________ atomic number.

a)

Increasing

b)

Decreasing

c)

Reducing

d)

Developing

68.

A ___________________ is a combination of two or more atoms that are held together by covalent bonds.

a)

Moles

b)

Ions

c)

Molecules

d)

Megatrons

69.
What is the Law of Conservation of mass?
a)
Mass is created in a chemical reaction
b)
Mass is created in a physical change
c)
New chemicals formed from a chemical reaction have a larger overall mass than the original reactants
d)
Mass is never created or destroyed
70.
The number to the lower side of an element is a 
a)
Subscript
b)
Superscript
c)
Coefficient
d)
Charge
71.
In a reaction A + B ----> C,  reactant A has 5g and product  C has 9g. How many grams does reactant B should have? 
a)
4g
b)
5g
c)
9g
d)
14g
72.
The number in front of a compound or element is a 
a)
Subscript
b)
Coefficient
c)
Superscript
d)
Charge
73.
How many nitrogen atoms does NH3 have?
a)
1
b)
2
c)
3
d)
4
74.
Bob puts 200 grams of ice into a pitcher with 900 grams of water. He gets distracted and comes back later to find that the ice has melted in the water. How many grams of water does Bob now have in the pitcher?
a)
200 g
b)
700 g
c)
1,100 g
75.
24 g of magnesium reacts with 38 g of fluorine to produce _____ g magnesium fluoride
a)
62 
b)
38
c)
24
d)
14
76.
What is the law of conservation of mass?
a)
The amount of matter changes when reacted or changed.
b)
The mass of all reactants are changed during a physical or chemical change
c)
The mass of the reactants equals the mass of the products
d)
The mass of the products is different than the mass of the reactants.
77.
When CaCO3 is heated, it forms CaO and CO2. Which of these statements best describes the mass of the products if 100 g of CaCO3 is heated?
a)
The difference in the products’ masses is equal to the mass of the CaCO3
b)
The sum of the products’ masses is less than the mass of the CaCO3
c)
The mass of each product is equal to the mass of the CaCO3
d)
The sum of the products’ masses equals the mass of the CaCO3
78.
The coefficient in  3H2O is
a)
6
b)
2
c)
3
d)
5
79.
The number of atoms of  N (nitrogen) in 3N2O5 is
a)
2
b)
5
c)
6
d)
15
80.

32 g of Oxygen completely reacts with 8 g of Hydrogen to produce _____ g Water

a)

8

b)

12

c)

24

d)

40

81.

Which Chemical Equation is Balanced?

a)

CH₄+O₂------CO₂+2H₂O

b)

H₂+O₂-----2H₂O₄

c)

4Al+3O₂-----2Al₂O₃

82.

Which Chemical Equation is Balanced?

a)

Fe4+O2------4FeO2+O2

b)

2H2+O2-----2H2O

c)

3Cr+4O₂-----2Cr₂O₃

83.

Which Chemical Equation is Balanced?

a)

4O2 + 2H2 + S2------ 2H2SO4

b)

4H2+O2-----2H2O2

c)

3Cr+4O₂-----2Cr₂O₃

84.

How many Sulfur atoms are present in the reactants of the following equation: 2SO2 + 2H2O2 ----> 2H2SO4

a)

2

b)

3

c)

4

d)

8

85.

How many Oxygen atoms are present in the product of the following equation: 2SO2 + 2H2O2 ----> 2H2SO4

a)

2

b)

3

c)

4

d)

8

86.

How many Hydrogen atoms are present in the product of the following equation: 2SO2 + 2H2O2 ----> 2H2SO4

a)

2

b)

3

c)

4

d)

8

87.

Which of the following are Subscripts in this Chemical Formula: 3Fe2O4

a)

3,4

b)

3,2

c)

2,4

d)

6

88.

The Coefficient (3) in the Chemical Formula, 3H2O, tells you how many _____________ there are.

a)

Atoms of Hydrogen

b)

Atoms of Oxygen

c)

Atoms of Water

d)

Molecules of Water

89.

The Subscript (2) in the Chemical Formula, 3H2O, tells you how many _____________ there are.

a)

Atoms of Hydrogen

b)

Atoms of Oxygen

c)

Atoms of Water

d)

Molecules of Water

90.

How many oxygen atoms are in this chemical formula?

a)

6 oxygen atoms

b)

2 oxygen atoms

c)

3 oxygen atoms

d)

4 oxygen atoms

91.

The law of conservation of mass states that matter cannot be created nor __________________.

a)

destroyed

b)

changed

c)

transferred

d)

rearranged

92.

It is best to observe the law of conservation of mass in a _____________________ because it will ensure that the mass is the same in the beginning and end of a chemical reaction.

a)

Partially open

b)

open system

c)

closed system

d)

balanced system

93.

In a closed system, a chemical reaction takes place. The mass of the reactants at the beginning of the reaction is 25g. What does the mass have to be at the end of the reaction in order to follow the law of conservation of mass?

a)

15g

b)

25g

c)

30g

d)

You can't tell with the given information.

94.

The following chemical equation occurs:

CH4 + 2O2 -> CO2 + 2H2O

Does this equation follow the law of conservation of mass?

a)

Yes

b)

No

c)

You can't tell with the given information

95.

Which Indian philosopher said Parmanu normally exist in combined form.

a)

Maharishi Kanad

b)

Chanakya

c)

Madhvacharya

d)

Pakudha Katyayama

96.

All matter is made of

a)

energy

b)

atoms

c)

electrons

d)

compounds

97.

What is an element?

a)

Two or more atoms joined together.

b)

One of over 100 types of atoms

c)

Two or more different elements joined together.

d)

A particle with no charge found in the nucleus of an atom.

98.

What is a molecule?

a)

two elements bonded together (sharing electrons)

b)

a mixture of different substances

c)

smallest individual particles

d)

salt mixed in water

99.

Which of the following is a chemical formula?

a)

H2SO4

b)

Si

c)

Hg

d)

C

100.
Explain the difference between an atom and a molecule.
a)
One molecule is made of one atom.
b)
One molecule is always made of different particles.
c)
One molecule is made of more than one atom.
d)
One molecule is made of more than two atoms.
101.
Explain the difference between an atom and a molecule.
a)
One molecule is made of one atom.
b)
One molecule is always made of different particles.
c)
One molecule is made of more than one atom.
d)
One molecule is made of more than two atoms.
102.
Explain the difference between an atom and a molecule.
a)
One molecule is made of one atom.
b)
One molecule is always made of different particles.
c)
One molecule is made of more than one atom.
d)
One molecule is made of more than two atoms.
103.
A single drop of water is made of approximately 1,670,000,000,000,000,000,000 molecules of water. When that same drop of water is heated it disappears. What happened to those molecules?
a)
The molecules are broken down to their smaller atoms hydrogen and oxygen and become part of the air.
b)
The molecules separate and become part of the air but remain water molecules.
c)
They are destroyed and no longer exist.
d)
They are turned into energy.
104.
Which of the models below represent a molecule? 
a)
A
b)
B
c)
C
d)
D
105.
Which of the models below represent an atom? 
a)
A
b)
B
c)
C
d)
D
106.
Elements are made of 
a)
many types of atoms 
b)
the periodic table
c)
one type of atom 
d)
molecules 
107.
All matter is made of 
a)
energy 
b)
atoms 
c)
electrons 
d)
compounds 
108.
What are the 3 particles that make-up the atom?
a)
protons, neutrons, and isotopes
b)
neutrons, isotopes, and electrons
c)
positives, negatives, and electrons
d)
protons, neutrons, and electrons
109.
What is the basic unit of matter and is the smallest particle of an element?
a)
Atoms
b)
Elements
c)
Compounds
d)
Molecules
110.
How many atoms are there in a molecule?
a)
no atoms
b)
1 or more atoms
c)
2 to thousands of atoms
d)
exactly 18 atoms
111.
Two or more atoms chemically bonded together are called a
a)
atom
b)
element
c)
molecule
d)
mixture
112.
How many carbon atoms are there in a methane molecule? 
a)
0
b)
1
c)
4
d)
5
113.
How many hydrogen atoms are there in a water molecule? 
a)
0
b)
1
c)
2
d)
3
114.
The repeating structure of table salt is in the shape of a
a)
pyramid
b)
snowflake
c)
hexagon
d)
cube
115.
What is the total number of atoms in an ammonia (NH3) molecule?
a)
1
b)
2
c)
3
d)
4
116.
Carbon dioxide (CO2) contains how many atoms of oxygen?
a)
0
b)
1
c)
2
d)
3
117.
What type of molecule does this picture show?
a)
hydrogen peroxide
b)
water
c)
carbon monoxide
d)
sugar
118.
Which one of these items has an extended structure with a pyramid shape?
a)
diamond
b)
gold
c)
glass
d)
salt
119.
How many hydrogen atoms are in a molecule of glucose/sugar (C6H12O6)?
a)
6
b)
12
c)
18
d)
24
120.
Which of these items is made up of one or more molecules?
a)
Gold
b)
Hydrogen
c)
Salt 
d)
Neon 
121.

What is a molecule?

a)

two elements bonded together (sharing electrons)

b)

a mixture of different substances

c)

smallest individual particles

d)

salt mixed in water

122.

According to Dalton's atomic theory, atoms are indestructible and indivisible. True or False?

a)

True

b)

False

123.

According to Dalton's atomic theory, different atoms are combined in fixed, whole number ratios to form _________

a)

Compounds

b)

Molecules

c)

Isotopes

d)

Mixtures

124.

According to Dalton's atomic theory, different atoms are combined in fixed, whole number ratios to form _________

a)

Compounds

b)

Molecules

c)

Isotopes

d)

Mixtures

125.

According to Dalton's atomic theory, different atoms are combined in fixed, whole number ratios to form _________

a)

Compounds

b)

Molecules

c)

Isotopes

d)

Mixtures

126.

Dalton took isotopes into account when developing his atomic theory. True or false?

a)

True

b)

False

127.

Which THREE postulates of Dalton's atomic theory have been proven false by later research?

a)

All matter is made up of atoms

b)

Atoms are indivisible and indestructible

c)

Atoms of different elements have different masses

d)

All atoms of the same element have identical properties

e)

Atoms combine in fixed, whole-number ratios to form compounds

128.

Mass of one atom of oxygen is.....

a)

166.032 x 1023 g\frac{16}{6.032\ x\ 10^{23}}\ g  

b)

32 / 6.023×1023  g32\ /\ 6.023\times10^{23\ \ }g  

c)

1 / 6.023×1023 g 1\ /\ 6.023\times10^{23\ g\ }  

d)

8μ8\mu  

129.

Mass of one atom of oxygen is.....

a)

166.032 x 1023 g\frac{16}{6.032\ x\ 10^{23}}\ g  

b)

32 / 6.023×1023  g32\ /\ 6.023\times10^{23\ \ }g  

c)

1 / 6.023×1023 g 1\ /\ 6.023\times10^{23\ g\ }  

d)

8μ8\mu  

130.

The Greek word "atomos" means _________

a)

Strong and indestructible

b)

Cannot be divided further

c)

Infinitesimally small

d)

Very brittle

131.

How many atoms are in 1 mole of Iodine (I)?

a)

6.022 x 1023

b)

4.022 x 1023

c)

6.022 x 1025

d)

4.022 x 1025

132.

What is Avogadro's number?

a)

6.02 x 1023

b)

1 mole

c)

600 million

d)

6.02

133.

How many moles are in 6.02 x 1023 molecules of H2O?

a)

1 mole

b)

2 moles

c)

6.02 moles

d)

602000000000000000000000 moles

134.

One mole of carbon dioxide (CO2) contains 6.02 x 1023 _____.

a)

atoms

b)

formula units

c)

ions

d)

molecules

135.

How many moles are in 8.30 X 1023 molecules of H2O?

a)

1.38 X 1023 moles H2O

b)

1.38 moles H2O

c)

2 moles H2O

d)

1 mole H2O

136.

How many molecules are there in 31.8 moles of water?

a)

5.28 x 10-23 molecules

b)

1.91 x 1025 molecules

c)

5.28x 10-25 molecules

d)

1.91 x 1023 molecules

137.

A mole is:

a)

The SI unit for mass

b)

The SI unit for the amount of a substance

c)

The SI unit for volume

d)

The SI unit for area

138.

What is the conversion factor that should be used to determine how many molecules are there in 4.00 moles of glucose, C6H12O6?

a)
b)
c)
d)
139.

What converting from moles to the number of particles, moles is multiplied by:

a)

an equivalent value

b)

a conversion factor

c)

the number of atoms in the formula

d)

the mass of the substance

140.

Which has the most particles?

a)

1 mole H2

b)

1 mole Na1+

c)

1 mole Al(OH)3

d)

These are all the same

141.

Why is the mole used in chemistry?

a)

The mass of atoms is in AMUs which is too hard to convert to grams.

b)

A dozen is not a scientific amount.

c)

Chemists needed to make chemistry easier to understand.

d)

It makes counting large numbers of small particles easier.

142.

SELECT ALL CORRECT ANSWERS - The mole can be used to measure:

a)

The amount of atoms in an element

b)

The amount of molecules in a covalent substance

c)

The amount of formula units in an ionic compound

d)

The amount of mass an object has

143.

How many moles there are in 5.68 x 1024 formula units of AlCl3?

a)

3.42 x 1024 moles

b)

9.44 x 1024 moles

c)

9.44 moles

d)

3.42 moles

144.

What is correct equation that should be used to determine how many molecules there are in 0.75 moles of (NH4)3PO4?

a)
b)
c)
d)
145.

What are the units for Avogadro's number?

a)

meters

b)

particles

c)

grams

d)

liters

146.

How many moles are in 4.5 x 1024 atoms of lithium?

a)

2.71 x 1048 particles

b)

7.47 moles

c)

7.47 x 1024 atoms

d)

2.71 moles

147.

How is moles abbreviated?

a)

M

b)

m

c)

mol

d)

ml

148.

What is the correct equation to determine how many calcium ions (Ca2+) in 2 moles?

a)
b)
c)
d)

This cannot be determined as calcium is not bonded.

149.

What is the correct equation to calculate the number of moles in 3.13 x 1026 molecules of H2O2?

a)
b)
c)
d)
150.

How many moles of Na contain 1.45 x 1021 atoms of Na?

a)

8.73 x 1044 moles

b)

8.73 moles

c)

0.00241 moles

d)

2.41 x 1044 moles

151.

What is the correct equation to calculate the number of moles in 3.13 x 1026 molecules of H2O2?

a)
b)
c)
d)
152.

According to whom each element had a characteristic atomic mass

a)

Proust

b)

Lavoisier

c)

Dalton

d)

Newton

153.

What is IUPAC

a)

International Union of Professional And Creative scientists

b)

International Union of Pure and Associated Chemistry

c)

International Union of Pure and Applied Chemists

d)

None of these

154.

Which element's atom was taken by scientists in the past to measure atomic mass

a)

Nitrogen

b)

Hydrogen

c)

Oxygen

d)

Chlorine

155.

In which year carbon-12 isotope was chosen as the standard reference for measuring atomic masses

a)

1978

b)

1982

c)

1961

d)

1954

156.

How were relative atomic masses determined

a)

Law of constant proportions and compounds formed

b)

Law of conservation of mass and compounds formed

c)

Laws of chemical combinations and compounds formed

d)

Dalton's atomic theory

157.

What is u

a)

Uniform mass

b)

Used mass

c)

Unified mass

d)

Unused mass

158.

Old atomic mass unit

a)

u

b)

amu

c)

IUPAC

d)

fmu

159.

Why was old atomic mass unit of the oxygen element considered relevant

a)

It reacted with a large number of elements and formed compounds

b)

It gave masses of most of the elements in rational numbers

c)

It gave masses of most of the elements in whole numbers

d)

Because it was artificially made

160.

Which element was chosen as the standard reference for measuring atomic masses

a)

Carbon

b)

Oxygen

c)

Carbon-12 isotope

d)

None of these

161.

Atomic Mass of calcium

a)

38

b)

27

c)

32

d)

40

162-174.

This video is about the history of chemical element symbols.

The video talks about how John Dalton, an English scientist, tried to name the various elements using pictorial symbols in the early 1800s. For example, the hydrogen element was represented as a circle with a dot at the center, oxygen was represented as a transparent circle, and carbon was represented as a shaded circle. However, these symbols were difficult to draw and remember, so they were soon replaced with a better system.

In 1813, John Jacob Berzelius devised a system using letters of the alphabet rather than signs. These symbols were much easier to write and remember. For example, the hydrogen element was represented by the letter H, the oxygen element was represented by the letter O, and the helium element was represented by the letters He. Today, we use a modified version of Berzelius's system, which is also known as the modern system for determining symbols of the elements.

162.

What is widely accepted in the field of chemistry?

a)

The modern system for element symbols

b)

The ancient system for element symbols

c)

The outdated system for element symbols

d)

The fictional system for element symbols

163.

What did John Dalton attempt to do in the early 1800s?

a)

Name chemical compounds

b)

Discover new elements

c)

Name elements using pictorial symbols

d)

Develop the periodic table

164.

Why was Berzelius's system with symbols like H for hydrogen and O for oxygen considered easier to write and remember?

a)

It used complex symbols that were difficult to understand

b)

It required memorizing long chemical names

c)

It used symbols that were not related to the element names

d)

It used simple symbols that were related to the element names

165.

What symbols did Dalton use for chemical elements?

a)

A square with a dot

b)

A circle with a dot

c)

A triangle with a dot

d)

A star with a dot

166.

What does the video provide a historical overview of?

a)

Evolution of chemical element symbols

b)

History of the periodic table

c)

Discovery of new elements

d)

Development of chemical formulas

167.

Who introduced a system using letters of the alphabet for element symbols in 1813?

a)

John Jacob Berzelius

b)

Antoine Lavoisier

c)

Dmitri Mendeleev

d)

Marie Curie

168.

What system is used to determine symbols of elements today?

a)

Dalton's system

b)

Mendeleev's system

c)

Berzelius's system

d)

Rutherford's system

169.

Who attempted to name chemical elements using pictorial symbols in the early 1800s?

a)
Dmitri Mendeleev
b)
Jöns Jacob Berzelius
c)
Marie Curie
d)
Antoine Lavoisier
170.

Which element was represented as a circle with a dot at the center in John Dalton's pictorial symbol system?

a)
Carbon
b)
Nitrogen
c)
Oxygen
d)
Hydrogen
171.

Why were John Dalton's pictorial symbols replaced with a better system?

a)
Lacked consistency and were not universally understood.
b)
Were difficult to draw accurately
c)
Were too colorful and distracting
d)
Did not include enough detail
172.

Who devised a system using letters of the alphabet to represent chemical elements?

a)
Isaac Newton
b)
Dmitri Mendeleev
c)
Albert Einstein
d)
Marie Curie
173.

What was the main advantage of John Jacob Berzelius's system over John Dalton's pictorial symbols?

a)
It used colors instead of letters.
b)
It included mathematical equations.
c)
It focused on compounds rather than elements.
d)
It used letters to represent elements.
174.

Which system for determining symbols of the elements do we use today?

a)
Alphabetical System
b)
Numerical System
c)
Color-Coding System
d)
Periodic Table System

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