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Questions and Answers
Which of the following best describes the trend of electronegativity on the periodic table?
Which of the following best describes the trend of electronegativity on the periodic table?
- Increases from right to left across a period and bottom to top in a group.
- Increases from right to left across a period and top to bottom in a group.
- Increases from left to right across a period and bottom to top in a group. (correct)
- Increases from left to right across a period and top to bottom in a group.
If two atoms have an electronegativity difference of 1.0, what type of bond is most likely to form between them?
If two atoms have an electronegativity difference of 1.0, what type of bond is most likely to form between them?
- Metallic bond
- Polar covalent bond (correct)
- Nonpolar covalent bond
- Ionic bond
Which element is considered the most electronegative?
Which element is considered the most electronegative?
- Oxygen (O)
- Fluorine (F) (correct)
- Chlorine (Cl)
- Sodium (Na)
What type of bond is formed when sodium (Na) completely transfers an electron to chlorine (Cl)?
What type of bond is formed when sodium (Na) completely transfers an electron to chlorine (Cl)?
In a water molecule (H₂O), why is the bond between oxygen and hydrogen considered polar covalent?
In a water molecule (H₂O), why is the bond between oxygen and hydrogen considered polar covalent?
What is the primary purpose of a Lewis dot structure?
What is the primary purpose of a Lewis dot structure?
According to the octet rule, how many valence electrons do most atoms 'want' in their outer shell to be stable?
According to the octet rule, how many valence electrons do most atoms 'want' in their outer shell to be stable?
What are 'lone pairs' in a Lewis dot structure?
What are 'lone pairs' in a Lewis dot structure?
If the electronegativity difference between two bonded atoms is 0.2, what type of bond is most likely to form?
If the electronegativity difference between two bonded atoms is 0.2, what type of bond is most likely to form?
Which type of bond is characterized by electrostatic attraction between oppositely charged ions?
Which type of bond is characterized by electrostatic attraction between oppositely charged ions?
How does the sharing of electrons differ between polar and nonpolar covalent bonds?
How does the sharing of electrons differ between polar and nonpolar covalent bonds?
Which of the following pairs of elements is most likely to form an ionic bond?
Which of the following pairs of elements is most likely to form an ionic bond?
Consider a molecule where one atom has a significantly higher electronegativity than the other. Which property is most likely to be observed in this molecule?
Consider a molecule where one atom has a significantly higher electronegativity than the other. Which property is most likely to be observed in this molecule?
Which force is primarily responsible for holding ions together in an ionic bond?
Which force is primarily responsible for holding ions together in an ionic bond?
If an atom has 7 valence electrons, how many more electrons does it need to satisfy the octet rule?
If an atom has 7 valence electrons, how many more electrons does it need to satisfy the octet rule?
In a Lewis dot structure, what does a single line between two atoms represent?
In a Lewis dot structure, what does a single line between two atoms represent?
What is the electronegativity difference range generally associated with a polar covalent bond?
What is the electronegativity difference range generally associated with a polar covalent bond?
Which of the following molecules is most likely to have nonpolar covalent bonds?
Which of the following molecules is most likely to have nonpolar covalent bonds?
If element X has a low electronegativity and element Y has a high electronegativity, what is the likely outcome when they bond?
If element X has a low electronegativity and element Y has a high electronegativity, what is the likely outcome when they bond?
How many lone pairs are present on the oxygen atom in a water molecule (H₂O) according to its Lewis dot structure?
How many lone pairs are present on the oxygen atom in a water molecule (H₂O) according to its Lewis dot structure?
Flashcards
Electronegativity
Electronegativity
An atom's measure of its tendency to attract electrons in a chemical bond.
Electronegativity trends
Electronegativity trends
Electronegativity increases from left to right across a period and from bottom to top in a group in the periodic table.
Most electronegative element
Most electronegative element
Fluorine (F) is the most electronegative element.
Ionic Bond
Ionic Bond
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Covalent Bond
Covalent Bond
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Nonpolar Covalent Bond
Nonpolar Covalent Bond
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Polar Covalent Bond
Polar Covalent Bond
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Lewis Dot Structure
Lewis Dot Structure
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Octet Rule
Octet Rule
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Study Notes
- Electronegativity describes an atom's propensity to attract electrons within a chemical bond.
- Elements increase in electronegativity from left to right across a period.
- Elements increase in electronegativity from bottom to top within a group.
- Fluorine (F) stands out as the most electronegative element.
Bond Types
- Electronegativity differences define bond types.
- Nonpolar covalent bonds occur when the electronegativity difference is between 0 and 0.4.
- Polar covalent bonds form when the electronegativity difference is between 0.5 and 1.7.
- Ionic bonds are likely to form when the electronegativity difference is greater than 1.7.
Ionic Bonds
- Ionic bonds occur through the complete transfer of electrons from one atom to another.
- These bonds typically form between a metal with low electronegativity and a nonmetal with high electronegativity.
- For Example: Sodium (Na) gives an electron to chlorine (Cl) to form Na⁺ and Cl⁻.
- Electrostatic attraction holds oppositely charged ions together.
Covalent Bonds
- Covalent bonds arise when atoms share electrons.
Types of Covalent Bonds
- Nonpolar covalent bonds arise from equal electron sharing due to similar or identical electronegativity.
- Polar covalent bonds are caused by unequal electron sharing, where one atom attracts electrons more strongly.
- For Example: In O-H, oxygen's higher electronegativity causes a polar covalent bond.
Lewis Dot Structure
- Lewis dot structures represent valence electrons as dots surrounding chemical symbols.
- They are used to illustrate bonding patterns in molecules.
- Atoms "want" a full outer shell of electrons, often 8, satisfying the octet rule.
- Shared electron pairs between atoms represent bonds.
- Unshared electron pairs are represented as dots.
- For Example: In H₂O, oxygen has 6 valence electrons, shares 2 with hydrogen atoms, and retains 2 lone pairs.
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