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Questions and Answers
What happens to the energy of an electron as it moves closer to the nucleus?
What happens to the energy of an electron as it moves closer to the nucleus?
What is the correct electron configuration for Calcium?
What is the correct electron configuration for Calcium?
Which type of bonding involves the transfer of electrons?
Which type of bonding involves the transfer of electrons?
Which group in the periodic table forms a +1 ion?
Which group in the periodic table forms a +1 ion?
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How many valence electrons does a Sodium atom have?
How many valence electrons does a Sodium atom have?
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For an ionic bond to form, what must be true about the electronegativity difference?
For an ionic bond to form, what must be true about the electronegativity difference?
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What characterizes covalent bonding?
What characterizes covalent bonding?
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What is the maximum number of electrons in the 3rd energy level?
What is the maximum number of electrons in the 3rd energy level?
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Study Notes
Electron Energy Levels
- Electron energy decreases when closer to the nucleus.
Electron Configuration of Calcium
- This information is not provided in the text.
Electron Orbital Diagram of Nitrogen
- This information is not provided in the text.
Valence Electrons
- Valence electrons are the outermost electrons involved in bonding.
- Energy levels and the maximum number of electrons they can hold are:
- 1st Energy Level: 2 electrons
- 2nd Energy Level: 8 electrons
- 3rd Energy Level: 18 electrons
- 4th Energy Level: 32 electrons
Types of Chemical Bonding
- Ionic Bonding: Transfer of electrons between nonmetals and metals.
- Covalent Bonding: Sharing of electrons between nonmetals.
- Metallic Bonding: Sea of electrons between metals.
Element Groups in the Periodic Table
- Element groups are listed in the periodic table.
- Group number, configuration, and number of valence electrons are shown in a table.
- Example: Group 1 elements (Na, Li) have 1 valence electron (s¹).
Chemical Bonding & Atoms
- Electrons jumping between energy levels produces colored light.
- Atoms bond to become stable or attain electronic configuration of a noble gas.
- Atoms bond to form compounds.
- Ionic bonds form when the electronegativity difference is greater than 1.9. Examples include NaCl, NaF, and KCl
- Anions gain electrons and become negatively charged.
- Cations lose electrons and become positively charged.
Group 1A (+1) Examples
- Sodium (Na)
- Lithium (Li)
Group 3 (+3) Examples
- Aluminum
Ionic Charges in Periodic Table
- Group 1A or Group I elements form +1 ions
- Group 3 elements form +3 ions
Covalent Bonding Examples
- Methane (CH4)
- Diamond (Carbon)
Properties of Ionic Compounds
- Form crystals
- Conduct electricity in aqueous solutions
- Hard and brittle
Properties of Covalent Molecular Compounds
- Soft and flexible
- Flammable
- Low melting and boiling points
Properties of Metals
- Malleable (can be shaped)
- Ductile (can be drawn into wires)
Conductivity & Malleability of Metals
- Metals are good electrical conductors due to a "sea" of free electrons within the lattice structure of metal ions.
Uses of Carbon Compounds
- Hydrocarbons are used as fuels (e.g., methane, butane).
- Other examples include: Isopropyl Alcohol, Ethyl Alcohol, Formalin, Acetone, Ethyne, Kerosene, Gasoline.
Alkanes
- Hydrocarbons with single bonds
- Examples: methane, ethane, propane, butane, pentane, octane.
- Octane has a higher boiling point than the other examples given
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Description
This quiz explores electron energy levels, configurations, and the different types of chemical bonding. Understand the significance of valence electrons and their role in forming ionic, covalent, and metallic bonds. Test your knowledge to see how these concepts relate to the periodic table and chemical behavior.
