SUBATOMIC PARTICLES.pptx. How to solve subatomic particles

SUBATOMIC PARTICLES.pptx. How to solve subatomic particles

1. Structure of the atoms

2. DAY 1

3. Lesson Outcomes Identify and label the subatomic particles in each atom diagram. Draw a basic atomic structure showing the nucleus and electron shells.

4. Let's Review!

5. W ho is known as the "father of modern atomic theory" for his work in developing the first atomic theory in the early 19th century?

6. J ohn Dalton

7. W hich scientist discovered the electron and proposed the "plum pudding" model of the atom?

8. J.J. Th omson

9. W ho conducted the gold foil experiment and discovered the nucleus, leading to the nuclear model of the atom?

10. Ernest Rutherf ord

11. W hich scientist is credited with discovering the neutron?

12. James Cha dwick

13. W ho proposed the planetary model of the atom, where electrons orbit the nucleus in fixed paths?

14. Neils Bohr

15. Atomic Theory Atomic theory is a scientific concept that explains the nature of matter and its behavior. Several theories try to explore the structure of atoms and their interactions with other atoms and molecules. Atomic theory has evolved over centuries with the contributions of many scientists.

16. Atomic Theory Solid Sphere Model of the Atom Atomism Plum Pudding Model of the Atom Nuclear Model of the Atom

17. Atomic Theory 01 ? 5th Century BC Atomism Atomism is a theory that was first proposed by the ancient Greek philosopher Democritus. According to atomism, all matter is made up of tiny, indivisible particles called atoms, which are in constant motion and are too small to be seen with the naked eye.

18. Atomic Theory 02 1803 Solid Sphere Model John Dalton's Solid Sphere Model of the Atom proposed this model as an attempt to describe the structure of the atom. According to this model, atoms are tiny, indestructible spheres with no internal structure. Solid Sphere Model of the Atom John Dalton

19. J.J. Thomson proposed that the atom is composed of a positively charged sphere with negatively charged electrons distributed throughout it. Atomic Theory 03 1904 Plum Pudding Model The negatively charged electrons were embedded in a positively charged "pudding" of matter, which made up most of the atom's mass. J.J. Thomson's Plum Pudding Model of the Atom electron

20. Ernest Rutherford proposed that most of the mass of the atom is concentrated in a tiny, positively charged nucleus at the center, with negatively charged electrons orbiting around it. Atomic Theory 04 1911 Nuclear Model This model became the basis for our understanding of atomic structure today. Ernest Rutherford’s Nuclear Model of the Atom electron nucleus

21. Atom and its Structure An atom is the basic unit of matter and the smallest particle of an element that retains its properties. Atoms are made up of three types of subatomic particles: protons, neutrons, and electrons.

22. Protons are positively charged particles located in the nucleus (center) of the atom Proton Atom and its Structure Electron Electrons are negatively charged particles that orbit around the nucleus. Neutron Neutrons are neutrally charged particles also located in the nucleus.

23. The nucleus of an atom is actually about 100,000 times smaller than the overall size of the atom. In perspective, if we imagine an atom were the size of a stadium, the nucleus would be smaller than a grain of sand. Atom and its Structure

24. W hat are some fundamental needs of modern daily life that might be influenced by atomic structure and nuclear technology?

25. Unlocking Content Vocabulary

26. Nucleus The nucl eus is the center of an atom. It contains two types of particles: protons and neutrons. The nucleus is very small and dense, holding most of the atom's mass.

27. Electron Shells Electron shell s surround the nucleus and are where electrons are found. These shells are layers at different distances from the nucleus. Electrons in these shells have negative charges and are involved in chemical reactions and bonding.

28. Protons (p⁺) Protons are particle s in the nucleus with a positive charge. Each proton has a mass of 1 atomic mass unit (amu). The number of protons in the nucleus determines the element and its atomic number.

29. Neutrons (n) Neutrons are particle s in the nucleus with no charge. They have a mass like protons, about 1 amu. Neutrons help stabilize the nucleus by reducing the repulsive forces between protons. The number of neutrons can vary in isotopes of the same element, changing the atomic mass without significantly altering chemical properties.

30. Electrons (e⁻) Electrons are negative ly charged particles found in electron shells around the nucleus. They have a very small mass compared to protons and neutrons, about 1/1836 of an amu. The arrangement of electrons determines the atom's reactivity, chemical properties, and bonding behavior.

31. Electrostatic Forces Electrostatic forces are the attractive or repu lsive forces between charged particles. In an atom, these forces keep negatively charged electrons orbiting around the positively charged protons in the nucleus of Subatomic Particles

32. Nuclear Forces Nuclear forces are the strong forces that hold protons and neutrons together in the nucleus of an atom. These forces are much stronger than electrostatic forces and ensure the nucleus stays intact despite the repulsive forces between positively charged protons.

33. Properties of Protons, Neutrons, and Electrons

34. Atoms are made o f three subatomic particles: protons, neutrons, and electrons. Each of them has unique properties.

35. Protons Charge: Posi tive (+1) Mass: 1 atomic mass unit (amu) Location: Inside the nucleus Symbol: p⁺

36. The number of protons determines the iden tity of the element. For example: An atom with 1 proton is hydrogen An atom with 6 protons is carbon An atom with 8 protons is oxygen This number is called the atomic number.

37. Neutrons Charge: Neu tral (0) Mass: About 1 amu (same as proton) Location: Inside the nucleus Symbol: n⁰

38. Neutrons add mass to the atom. They help stabilize the nucleus (keep pro tons from repelling each other). Atoms with the same number of protons but different numbers of neutrons are called isotopes.

39. Electrons Charge: Negative (–1) Mass: Very tiny (about 1/1836 amu) Location: Outside the nucleus, i n electron shells or energy levels Symbol: e⁻

40. Electrons are responsible for chemical bonding and reactivity. In a neutral atom, the number of electrons = number of protons.

41. How to Know the Number of Protons, Electrons, and Neutrons

42. Number of Protons = Atomic Number The atomic number (usually the small whole number above the element symbol) tells you the number of protons in an atom.

43. Number of Electrons = Number of Protons (in a Neutral Atom) Atoms are n eutral, so they have the same number of electrons and protons.

44. Number of Neutrons = Mass Number – Atomic Number

45. Activity 1: Completing the Table of Subatomic Particles

46. Fill in the following table with the properties of subatomic particles.

47. Write the atomic number, number of protons, neutrons, and electrons of the following elements.

48. How do the number of protons, neutrons, and electrons define the properties of an element?

49. Why is the location of protons, neutrons, and electrons within an atom important for its stability?

50. How do the charges of subatomic particles contribute to the overall charge of an atom?

51. What are the components of an atom? What are their functions?

52. What are the components of an atom? What are their functions?

53. Which part of the atom contains protons and neutrons? A. Electron shell B. Nucleus C. Orbit D. Energy level

54. What is the charge of an electron? A. Positive B. Neutral C. Negative D. None

55. Which subatomic particle determines the atomic number? A. Neutron B. Proton C. Electron D. Isotope

56. Where are electrons located in an atom? A. Inside the nucleus B. In the electron shells C. In the neutron cloud D. Between protons

57. What is the function of neutrons? A. Give atoms energy B. Add color C. Stabilize the nucleus D. Create electricity

58. -Each group will create a poster about their assigned particle. The poster should include: - The particle’s charge (positive, negative, or neutral) - The particle’s relative mass

59. - The particle’s location within the atom - The particle’s role/function in the atom - Any interesting facts or historical information about the particle

60. DAY 2

61. Properties of Subatomic Particles: Protons, Neutrons, Electrons

62. Let's Review!

63. W hat do you know about protons?

64. W hich particle is negatively charged?

65. W hy is the discovery of the electron significant in understanding atomic structure?

66. T he discovery of the electron revealed that atoms have internal structure and are not indivisible, leading to the development of modern atomic theory and understanding of chemical reactions.

67. How does the location of electrons affect the chemical behavior of an element?

68. El ectrons in the outermost energy levels (valence electrons) determine an element’s chemical reactivity and bonding properties, influencing how elements interact to form compounds.

69. Explain how the electron cloud model provides a more accurate representation of electron location compared to Thomson's initial model.

70. The el ectron cloud model depicts electrons in probabilistic orbitals rather than fixed paths, reflecting the uncertainty and distribution of electrons around the nucleus more accurately than Thomson’s “plum pudding” model.

71. Activity 2: Understanding Atomic Structure

72. What are the diff erences among protons, neutrons, and electrons?

73. What is the cha rge of a neutron? A. +1 B. -1 C. 0 D. +2

74. Where is a proton locat ed? A. Electron shell B. Outside atom C. Nucleus D. Electron cloud

75. What is the approximate mass of a proton ? A. 0 B. 1 amu C. 0.5 amu D. 2 amu

76. What does the number of electrons affect ? A. Temperature B. Light absorption C. Chemical bonding D. Size

77. What subatomic particle identifies an element ? A. Neutron B. Proton C. Electron D. Isotope

78. DAY 3

79. Let's Review!

80. Interaction and Significance of Subatomic Particles

81. Why do you think electrons do not crash into the nucleus despite their attraction to protons?

82. Because the electrons are moving very fast around the nucleus. Their motion creates a balance between the attractive force pulling them toward the nucleus and the energy they have from moving. It’s like how planets orbit the sun—they don’t fall in because of their speed.

83. How might these forces affect the stability of an atom?

84. The electrostatic attraction between protons and electrons helps keep the electrons in place around the nucleus, so the atom stays together. If this force was too strong or too weak, the atom could fall apart or not form at all.

85. What might happen to the nucleus if there were no neutrons?

86. If there were no neutrons, the protons would all repel each other because they have the same positive charge. The nucleus would be unstable and could break apart.

87. Why are these forces crucial for the nucleus?

88. These nuclear forces act like glue to hold the protons and neutrons together in the nucleus. Without them, the nucleus wouldn’t stay together, and atoms couldn’t exist properly.

89. Electrostatic Forces – Why Electrons Stay Around the Nucleus Electrons are negatively charged, and protons in the nucleus are positively charged. Opposite charges attract, so the electrons are pulled toward the nucleus. But because electrons are moving really fast, they don’t fall in—they keep circling around the nucleus, kind of like how the moon orbits the Earth. How Atoms Stay Together?

90. Inside the nucleus, there are protons (positive) and neutrons (no charge). Protons want to push away from each other because they have the same charge. But neutrons help hold them together using strong nuclear force—a powerful "glue" that keeps the nucleus stable. Nuclear Forces – Why the Nucleus Stays Together

91. Protons give the atom its identity and are needed in the nucleus. Neutrons help stop the protons from pushing each other apart. Stability of the Atom

92. If electrostatic force was too strong or too weak, electrons might crash into the nucleus or fly away. If nuclear force was missing, the protons would repel each other and the nucleus would fall apart. That’s why atoms need a perfect balance of these forces to stay together and be stable! What If These Forces Weren’t Balanced?

93. Electrons are kept in orb it by their energy and the balance of forces. Key ideas:

94. Balanced forces keep the atom stable; imbalance can make it unstable. Key ideas:

95. Without neutrons, pro tons would repel each other, causing the nucleus to break apart. Key ideas:

96. Nuclear forces keep pro tons and neutrons together, ensuring nucleus stability. Key ideas:

97. Activity 3: Role of Subatomic Particles and Atomic Stability

98. PRESENTATION OF OUTPUT

99. Balanced nuclear forces keep atoms stable. Too few/many neutrons = instability.

100. What keeps electrons from falling into the nucleus? A. Gravity B. Electrostatic attraction and their energy C. Neutron repulsion D. Magnetic field

101. What force holds protons and neutrons together? A. Electrostatic force B. Magnetic force C. Gravitational force D. Nuclear force

102. What happens if an atom has too many neutrons? A. It becomes larger B. It is more stable C. It becomes radioactive D. It gets smaller

103. What happens if an atom has too many neutrons? A. It becomes larger B. It is more stable C. It becomes radioactive D. It gets smaller

104. What is the role of neutrons? A. Identify the element B. Keep nucleus stable C. Give energy D. Bond with electrons

105. Why don’t protons repel each other in the nucleus? A. They are neutral B. They are attracted to electrons C. Nuclear forces overcome repulsion D. They’re far apart

106. DAY 4

107. Let's Review!

108. What is the outermost part of an atom?

109. Have you heard of valence electrons before? What do you think they do?

110. Sodium vs. Helium

111. Sodium (Na) Electron Arrangement: 2, 8, 1 Valence Electrons: 1 Reactivity: Very reactive

112. Sodium has only 1 valence electron. It "wants" to lose this electron to become stable (like noble gases with full outer shells).

113. This makes it highly reactive, especially with substances like water. When sodium contacts water, it reacts explosively, releasing hydrogen gas and heat.

114. Real-World Example: Sodium is stored in oil in laboratories to prevent contact with moisture.

115. Real-World Example: Sodium compounds (like table salt—NaCl) are safe because sodium has already reacted and formed a stable compound.

116. Helium (He) Electron Arrangement: 2 (only one shell, which is full) Valence Electrons: 2 Reactivity: Very stable (inert)

117. Helium already has a full outer shell, so it does not need to gain or lose electrons. It does not form compounds easily and is considered chemically inert.

118. Real-World Example: Helium is used in balloons and airships because it is non-flammable and safe, unlike hydrogen, which is reactive and flammable.

119. Real-World Example: Also used in cooling MRI machines and deep-sea diving tanks due to its stability and lightness.

120. The number of valence electrons determines how reactive an element is: 1 or 7 valence electrons = highly reactive (e.g., Sodium, Chlorine) Full outer shell (like 2 or 8) = stable/inert (e.g., Helium, Neon)

121. What Are Valence Electrons?

122. Valence electrons are the electrons found in the outermost shell (energy level) of an atom.

123. They are the electrons involved when atoms form bonds with other atoms.

124. The number of valence electrons determines how reactive an element is.

125. How Do Valence Electrons Affect Reactivity?

126. Atoms want to be stable, and to do that, they try to have a full outer shell of electrons (usually 8, known as the "octet rule").

127. Atoms with 1, 2, or 3 valence electrons tend to lose them to become stable. These are usually metals (e.g., Sodium).

128. Atoms with 5, 6, or 7 valence electrons tend to gain or share electrons. These are often nonmetals (e.g., Oxygen, Chlorine).

129. Atoms with a full outer shell (like 8 valence electrons) are nonreactive or inert—they don’t need to gain or lose anything.

130. Noble gases are elements in Group 18 of the periodic table (e.g., Helium, Neon, Argon). They have full outer electron shells.

131. Helium has 2 electrons (1st shell is full with 2) Neon has 8 electrons in its outer shell (2, 8) Argon has 8 valence electrons (2, 8, 8)

132. Because their outer shells are already full, noble gases do not need to bond with other elements. That’s why they are chemically stable and rarely form compounds.

133. Activity 4: Investigatory Case Study – The Mystery of the Unstable Atom

134. PRESENTATION OF OUTPUT

135. The number of valence electrons determines how an element bonds with others. Full shells = stability.

136. What are valence electrons? A. Electrons in the nucleus B. Electrons in the outermost shell C. Electrons with no charge D. Electrons in pairs

137. Why are noble gases unreactive? A. They have no electrons B. They are heavy C. Their outer shells are full D. They have more protons

138. Which element is most reactive due to having one valence electron? A. Neon B. Oxygen C. Sodium D. Helium

139. What happens when atoms with incomplete outer shells react? A. They explode B. They gain or lose protons C. They form bonds D. They become unstable

140. Which electron arrangement is most stable? A. 2, 1 B. 2, 8 C. 2, 6 D. 2, 7

141. DAY 5

142. Let's Review!

143. What is the structure of an atom?

144. What is the role of each subatomic particle?

145. GROUP ACTIVITY

146. Why is each subatomic particle important?

147. What would happen if one was missing?

148. Which subatomic particle is the most important and why? Support your choice with scientific reasoning.

149. All atoms are made up of protons, neutrons, and electrons.

150. Their arrangement and properties determine the element’s stability and behavior.

151. Which subatomic particle has a negative charge? A. Proton B. Electron C. Neutron D. Nucleus

152. What does the atomic number represent? A. Number of neutrons B. Number of electrons only C. Number of protons D. Total mass

153. Which of the following contributes to the atom’s mass and is neutral? A. Proton B. Neutron C. Electron D. Shell

154. Why do electrons stay around the nucleus? A. Gravity pulls them B. Nuclear force keeps them C. Electrostatic attraction D. They are glued

155. What is the most important reason for atomic stability? A. Presence of energy B. Size of atom C. Balanced subatomic forces D. Shape of atom