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Samira Tasnim

2/20/2023

Chemistry

Chemistry Unit 4 - Chemical Bonding

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Atomic Structure and Properties

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Valence Electrons and Ionic Compounds

Cool Chemical Reactions: Keeping the Balance!

Chemical bonding and reactions are fundamental processes that follow precise rules of conservation and energy exchange. Conservation of mass energy and charge in chemical reactions governs all chemical transformations, while endothermic and exothermic processes in chemical bonding determine energy flow. The formation and characteristics of ionic and covalent bonds create diverse molecular structures.

• Chemical bonds form through electron transfer (ionic) or sharing (covalent), following conservation principles
• Bond formation releases energy (exothermic) while breaking requires energy (endothermic)
• Molecular polarity depends on electron distribution and affects physical properties
• Bonding type determines material characteristics like conductivity and melting point
• Atoms seek stable electron configurations through various bonding mechanisms

...

2/20/2023

186

1. All chemical reactions show conservation of mass, energy, and charge ● Breaking a chemical bond is an endothermic process • Forming a che

View

Energy Changes in Chemical Reactions

This page explores the energy dynamics of chemical reactions and molecular polarity. It details how bonds store and release energy during chemical processes.

Definition: Endothermic reactions absorb energy from surroundings, while exothermic reactions release energy to surroundings.

Highlight: The BARF principle BrokenAbsorbed,ReleasedFormedBroken Absorbed, Released Formed explains energy changes in reactions.

Example: When hydrogen molecules H2H₂ break apart, they absorb energy endothermicendothermic, while when iodine atoms combine to form I₂, they release energy exothermicexothermic.

Vocabulary: Electronegativity is a measure of an atom's ability to attract electrons in a chemical bond.

The page also covers molecular polarity principles and the SNAP rule for determining molecular polarity.

1. All chemical reactions show conservation of mass, energy, and charge ● Breaking a chemical bond is an endothermic process • Forming a che

View

Covalent Bonding Mechanisms

This page delves into the specifics of covalent bonding and molecular structure formation. It explains how nonmetals share electrons to achieve stable configurations.

Definition: Covalent bonds form when two nonmetals share valence electrons, with the electronegativity difference being less than 1.7.

Example: The formation of water molecules demonstrates covalent bonding where oxygen shares electrons with two hydrogen atoms.

Highlight: Multiple covalent bonds can form when atoms share more than one pair of electrons.

Vocabulary: Lewis dot diagrams are representations showing valence electrons as dots around atomic symbols.

The page includes step-by-step instructions for writing covalent bond formulas and understanding electron sharing patterns.

1. All chemical reactions show conservation of mass, energy, and charge ● Breaking a chemical bond is an endothermic process • Forming a che

View

Advanced Bonding Concepts

This final page expands on covalent bonding principles and multiple bond formation. It focuses on the sharing of electron pairs and resulting molecular structures.

Definition: Multiple covalent bonds involve sharing more than one pair of electrons between atoms.

Example: Oxygen molecules O2O₂ form double bonds by sharing two pairs of electrons.

Highlight: Group 16 elements oxygenfamilyoxygen family commonly form multiple covalent bonds.

The page emphasizes how different types of covalent bonds affect molecular properties and stability.

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Subjects

Chemistry

Atomic Structure and Properties

Valence Electrons and Ionic Compounds

 

Chemistry

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186

•

Feb 20, 2023

•

4 pages

Cool Chemical Reactions: Keeping the Balance!

user profile picture

Samira Tasnim

@s.amiraa

Chemical bonding and reactions are fundamental processes that follow precise rules of conservation and energy exchange. Conservation of mass energy and charge in chemical reactions governs all chemical transformations, while endothermic and exothermic processes in chemical bondingdetermine energy flow.... Show more

1. All chemical reactions show conservation of mass, energy, and charge ● Breaking a chemical bond is an endothermic process • Forming a che

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Energy Changes in Chemical Reactions

This page explores the energy dynamics of chemical reactions and molecular polarity. It details how bonds store and release energy during chemical processes.

Definition: Endothermic reactions absorb energy from surroundings, while exothermic reactions release energy to surroundings.

Highlight: The BARF principle BrokenAbsorbed,ReleasedFormedBroken Absorbed, Released Formed explains energy changes in reactions.

Example: When hydrogen molecules H2H₂ break apart, they absorb energy endothermicendothermic, while when iodine atoms combine to form I₂, they release energy exothermicexothermic.

Vocabulary: Electronegativity is a measure of an atom's ability to attract electrons in a chemical bond.

The page also covers molecular polarity principles and the SNAP rule for determining molecular polarity.

1. All chemical reactions show conservation of mass, energy, and charge ● Breaking a chemical bond is an endothermic process • Forming a che

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Access to all documents

Improve your grades

Join milions of students

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Covalent Bonding Mechanisms

This page delves into the specifics of covalent bonding and molecular structure formation. It explains how nonmetals share electrons to achieve stable configurations.

Definition: Covalent bonds form when two nonmetals share valence electrons, with the electronegativity difference being less than 1.7.

Example: The formation of water molecules demonstrates covalent bonding where oxygen shares electrons with two hydrogen atoms.

Highlight: Multiple covalent bonds can form when atoms share more than one pair of electrons.

Vocabulary: Lewis dot diagrams are representations showing valence electrons as dots around atomic symbols.

The page includes step-by-step instructions for writing covalent bond formulas and understanding electron sharing patterns.

1. All chemical reactions show conservation of mass, energy, and charge ● Breaking a chemical bond is an endothermic process • Forming a che

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Advanced Bonding Concepts

This final page expands on covalent bonding principles and multiple bond formation. It focuses on the sharing of electron pairs and resulting molecular structures.

Definition: Multiple covalent bonds involve sharing more than one pair of electrons between atoms.

Example: Oxygen molecules O2O₂ form double bonds by sharing two pairs of electrons.

Highlight: Group 16 elements oxygenfamilyoxygen family commonly form multiple covalent bonds.

The page emphasizes how different types of covalent bonds affect molecular properties and stability.

1. All chemical reactions show conservation of mass, energy, and charge ● Breaking a chemical bond is an endothermic process • Forming a che

Sign up to see the contentIt's free!

Access to all documents

Improve your grades

Join milions of students

By signing up you accept Terms of Service and Privacy Policy

Fundamentals of Chemical Bonding

This page introduces core concepts of chemical bonding and conservation principles. Chemical reactions consistently demonstrate conservation of mass, energy, and charge while following specific bonding patterns.

Definition: Chemical bonds form when valence electrons are either transferred between atoms ionicionic, shared between atoms covalentcovalent, or exist in a free-moving electron sea metallicmetallic.

Highlight: Atoms achieve stability by obtaining a full valence electron shell, typically requiring 8 electrons exceptforHandHewhichneed2except for H and He which need 2.

Example: Sodium chloride NaClNaCl demonstrates ionic bonding where sodium transfers an electron to chlorine.

Vocabulary: Valence electrons are the outermost electrons of an atom that participate in chemical bonding.

The page includes detailed diagrams showing electron configurations and bonding patterns, emphasizing how electronegativity differences determine bond types.

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Stefan S

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This app is really great. There are so many study notes and help [...]. My problem subject is French, for example, and the app has so many options for help. Thanks to this app, I have improved my French. I would recommend it to anyone.

Samantha Klich

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I think it’s very much worth it and you’ll end up using it a lot once you get the hang of it and even after looking at others notes you can still ask your Artificial intelligence buddy the question and ask to simplify it if you still don’t get it!!! In the end I think it’s worth it 😊👍 ⚠️Also DID I MENTION ITS FREEE YOU DON’T HAVE TO PAY FOR ANYTHING AND STILL GET YOUR GRADES IN PERFECTLY❗️❗️⚠️

Thomas R

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Brad T

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Not only did it help me find the answer but it also showed me alternative ways to solve it. I was horrible in math and science but now I have an a in both subjects. Thanks for the help🤍🤍

David K

iOS user

The app's just great! All I have to do is enter the topic in the search bar and I get the response real fast. I don't have to watch 10 YouTube videos to understand something, so I'm saving my time. Highly recommended!

Sudenaz Ocak

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Greenlight Bonnie

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I found this app a couple years ago and it has only gotten better since then. I really love it because it can help with written questions and photo questions. Also, it can find study guides that other people have made as well as flashcard sets and practice tests. The free version is also amazing for students who might not be able to afford it. Would 100% recommend

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Marco B

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THE QUIZES AND FLASHCARDS ARE SO USEFUL AND I LOVE THE SCHOOLGPT. IT ALSO IS LITREALLY LIKE CHATGPT BUT SMARTER!! HELPED ME WITH MY MASCARA PROBLEMS TOO!! AS WELL AS MY REAL SUBJECTS ! DUHHH 😍😁😲🤑💗✨🎀😮

Elisha

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This app is phenomenal down to the correct info and the various topics you can study! I greatly recommend it for people who struggle with procrastination and those who need homework help. It has been perfectly accurate for world 1 history as far as I’ve seen! Geometry too!

Paul T

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