2. Atoms & Elements

Subatomic Particles

Protons, Neutrons, and Electrons (Intro to Subatomic Particles!)

Subtracting the atomic number (found on a periodic table) from the given mass number determines the number of neutrons.

Correct, this isotope of Cl has 18 neutrons.

 The sum of the number of neutrons and protons in an atom is called the mass number. 

Which of the following has the largest number of neutrons?

Atoms contain an equal number of protons and neutrons.

Some isotopes have equal numbers of protons and neutrons but many do not.

Protons, found in the nucleus of an atom, have no net charge.

The charge on protons causes the repulsion of the alpha particles in Rutherford's experiment.

Electrons, found outside the nucleus, have a positive charge.

The positive charge of the atom is contained in the nucleus.

Neutrons, found in the nucleus, have a neutral charge.

Correct, the name "neutron" is derived from the term "neutral".

Protons, neutrons, and electrons all have similar masses.

Only two of the types of subatomic particles have similar masses.

Which of the following statements is true?

Fill in the gaps in the following table, assuming each column
represents a neutral atom.
Symbol 89Y
Protons 78 89
Neutrons 123
Electrons 81 50
Mass no. 195 119 227
Complete the second row of the table.

What is an Atom? (Structure and Subatomic Particles)

The Subatomic Particles

Calculating the Protons, Neutrons and Electrons for an Atom

Nuclide Symbols: Atomic Number, Mass Number, Ions, and Isotopes

Fill in the gaps in the following table, assuming each column
represents a neutral atom.
Symbol 159Tb 
Protons 29 37 
Neutrons 34 53 
Electrons 42 34 
Mass no. 79 85
Complete the fifth row of the table.

Which of the following three drawings represents a neutral Na atom?
(a) 
(b) 
(c)

Determine whether each of the following statements is true
or false. If false, correct the statement to make it true: (a) The
nucleus has most of the mass and comprises most of the volume
of an atom.

(a) Define atomic number and mass number.

Most of an atom&#8217;s mass and all of its negative charge are contained in a small core called the nucleus.

Correct, the nucleus is positively charged.

Most of the volume of an atom is empty space, through which electrons are dispersed.

This statement is part of Rutherford's nuclear theory.

 Rutherford proposed this theory based on the results of his gold foil experiment. 

Which of the following statements about the nuclear theory of atoms is false?

Determine whether each of the following statements is true
or false. If false, correct the statement to make it true: (b) Every atom of a given element has the
same number of protons.

Consider an atom of 32P. (c) What is the symbol of the atom obtained by adding one 
neutron to 32P?

Consider an atom of 32P. (a) How many protons, neutrons,
and electrons does this atom contain?

How to find the number of protons, neutrons, and electrons from the periodic table

Determine whether each of the following statements is true 
or false. If false, correct the statement to make it true: (c) The number of electrons in an 
atom equals the number of neutrons in the atom.

Identify the element represented by each of the following
symbols and give the number of protons and neutrons in
each: (a) 115 X
Identify the element.

In terms of size, neutrons are the largest, protons are slightly smaller, and the electrons are the smallest.

If the charge and mass of one proton is 1.60218 x 10-19&nbsp;C and 1.673 x 10-30 g respectively, what is the charge of 378 kg of protons?

Fill in the gaps in the following table, assuming each column
represents a neutral atom.
Symbol 89Y 
Protons 78 89 
Neutrons 123 
Electrons 81 50 
Mass no. 195 119 227
Complete the first row of the table.

Subatomic Particles of an Atom | Chemistry

Which statements about subatomic particles are true? 
a. If an atom has an equal number of protons and electrons, it will be charge-neutral. 
b. Electrons are attracted to protons. 
c. Electrons are much lighter than neutrons. 
d. Protons have twice the mass of neutrons.

A helium nucleus has two protons and two neutrons. How
many electrons does it take to equal the mass of a helium
nucleus?

How many protons, neutrons, and electrons are in the 
following atoms? (e) 239U

Consider an atom of 32P. (b) What is the symbol
of the atom obtained by adding one proton to 32P?

What is the difference between an atom’s atomic number and its mass number?

According to the table above, how many electrons are required to produce a charge of –2.0 C?

How many electrons does it take to equal the mass of a proton?

(b) Which of these can vary without changing the identity of the element?

Consider an atom of 58Ni. (a) How many protons, neutrons,
and electrons does this atom contain?

Fill in the gaps in the following table, assuming each column
represents a neutral atom.
Symbol 159Tb 
Protons 29 37 
Neutrons 34 53 
Electrons 42 34 
Mass no. 79 85
Complete the third row of the table.

Which statements about subatomic particles are false? 
a. Protons and electrons have charges of the same magnitude but opposite sign. 
b. Protons have about the same mass as neutrons. 
c. Some atoms don’t have any protons. 
d. Protons and neutrons have charges of the same magnitude but opposite signs.

How many protons, neutrons, and electrons are in the 
following atoms? (c) 59Co

How many protons, neutrons, and electrons are in the 
following atoms? (d) 55Mn

Subatomic Particles Example 1

Atomic Number, Atomic Mass, and the Atomic Structure | How to Pass Chemistry

On a dry day, your body can accumulate static charge from
walking across a carpet or from brushing your hair. If your body
develops a charge of -15 mC (microcoulombs), how many excess
electrons has it acquired?

How to find the Protons Neutrons and Electrons of an element on the Periodic table

Robert Millikan's oil drop experiment characterized the charge of an electron.

Correct, based on his oil-drop experiment.

Who is given credit for determining the charge of an electron?

How many protons, neutrons, and electrons are present in an atom of 2 206Pb? (LO 2.14)
(a) 82 protons, 206 neutrons, 82 electrons 
(b) 124 protons, 82 neutrons, 124 electrons 
(c) 82 protons, 124 neutrons, 82 electrons 
(d) 82 protons, 82 neutrons, 124 electrons

Fill in the gaps in the following table, assuming each column
represents a neutral atom.
Symbol 159Tb 
Protons 29 37 
Neutrons 34 53 
Electrons 42 34 
Mass no. 79 85
Complete the second row of the table excluding the row with isotope symbol.

Fill in the gaps in the following table, assuming each column
represents a neutral atom.
Symbol 89Y
Protons 78 89
Neutrons 123
Electrons 81 50
Mass no. 195 119 227
Complete the third row of the table.

Identify the element represented by each of the following
symbols and give the number of protons and neutrons in
each: (b) 7533X
Identify the element.
Give the number of protons and neutrons.

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1. Intro to General Chemistry

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Millikan Oil Drop Experiment

The Oil Drop Experiment helped with determining the fundamental charge of the electron.&nbsp;

Ions

Ions represent elements that possess either a positive charge or a negative charge.&nbsp;

Periodic Table: Charges

Elements lose or gain electrons to have the ideal number of outer shell electrons like the noble gases.&nbsp;

Law of Definite Proportions

"Different samples of a pure chemical compound always contain the same proportions of elements by mass."

Periodic Table: Classifications

The Periodic Table contains 3 Major Classifications when describing its elements

Isotopes

Isotopes are atoms of an element that have the same atomic number, but different mass number.&nbsp;

The Atom

The atom represents the basic functional unit in chemistry

Mole Concept

The Mole Concept involves the interconversions between different unit amounts of a substance.

Periodic Table: Representative Elements & Transition Metals

The Groups of the Periodic Table can be broken down into the Representative Elements and Transition Metals

Atomic Theory

John Dalton, one of the "Fathers of Chemistry"is credited with modernizing the Atomic Theory.

The atom is composed of 3 subatomic particles:neutrons, protons, and electrons.

Periodic Table: Elemental Forms

The elements of the Periodic Table exist in different elemental forms in the natural world

Periodic Table: Phases

Under standard conditions of temperature and pressure, the elements can exist as solids, liquids or gases

Atomic Mass

The atomic mass of an element includes the masses of all 3 subatomic particles of neutrons, protons and electrons.&nbsp;

Periodic Table: Group Names

The Periodic Table can be further classified into Periods and Groups.&nbsp;

Law of Conservation of Mass

"In a chemical reaction, no matter is created or destroyed, but instead changes form."

Calculating Molar Mass

Molar Mass is a physical property that represents the mass of a substance divided by the amount of that substance.

Rutherford Gold Foil Experiment

The Gold Foil Experiment helped with the discovery of the positively charged nucleus.

Law of Multiple Proportions

“When 2 elements (A &amp; B) form different compounds, the mass of Element B that combine with 1 g of A are a ratio of whole numbers."

Periodic Table: Element Symbols

The Element Symbols of the Periodic Table represent the abbreviated form of an element