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What is the general equation for acid-base reactions?
What is the general equation for acid-base reactions?
Which of the following is a strong acid?
Which of the following is a strong acid?
What is the purpose of an indicator in acid-base reactions?
What is the purpose of an indicator in acid-base reactions?
Which of the following is a physical property of acids?
Which of the following is a physical property of acids?
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What is a chemical property of bases?
What is a chemical property of bases?
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What is the product of an acid-base reaction between HCl and NaOH?
What is the product of an acid-base reaction between HCl and NaOH?
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What is the trend of electronegativity across a period of the periodic table?
What is the trend of electronegativity across a period of the periodic table?
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Which of the following elements has the highest electron affinity?
Which of the following elements has the highest electron affinity?
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What is the trend of ionization potential across a period of the periodic table?
What is the trend of ionization potential across a period of the periodic table?
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Which of the following elements has the lowest electronegativity?
Which of the following elements has the lowest electronegativity?
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What is the trend of atomic radius across a period of the periodic table?
What is the trend of atomic radius across a period of the periodic table?
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Which of the following elements has the highest atomic radius?
Which of the following elements has the highest atomic radius?
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What is the relationship between electron affinity and electronegativity?
What is the relationship between electron affinity and electronegativity?
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Which of the following elements has the lowest ionization potential?
Which of the following elements has the lowest ionization potential?
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What is the number of electrons present in the valence shell of halogen?
What is the number of electrons present in the valence shell of halogen?
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What is the correct configuration for an element A belonging to period 3 and Group II?
What is the correct configuration for an element A belonging to period 3 and Group II?
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What happens to the atomic size of elements on moving from left to right across a period of the periodic table?
What happens to the atomic size of elements on moving from left to right across a period of the periodic table?
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What is the trend of non-metallic character of elements on moving from left to right across a period of the periodic table?
What is the trend of non-metallic character of elements on moving from left to right across a period of the periodic table?
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What happens to the ionization potential of elements on moving from left to right across a period of the periodic table?
What happens to the ionization potential of elements on moving from left to right across a period of the periodic table?
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Why does ionization potential increase over a period from left to right?
Why does ionization potential increase over a period from left to right?
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What happens to the electron affinity of elements in groups 1 to 7 on moving from left to right across a period of the periodic table?
What happens to the electron affinity of elements in groups 1 to 7 on moving from left to right across a period of the periodic table?
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Which element in period 3 has a zero electron affinity?
Which element in period 3 has a zero electron affinity?
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What is the general trend of atomic size as we move left to right across a period?
What is the general trend of atomic size as we move left to right across a period?
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Which of the following is true about the metallic character of elements in a group?
Which of the following is true about the metallic character of elements in a group?
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What is the general trend of ionization potential across a period?
What is the general trend of ionization potential across a period?
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What is the relationship between electron affinity and chemical reactivity of non-metals?
What is the relationship between electron affinity and chemical reactivity of non-metals?
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What is the general trend of electronegativity across a period?
What is the general trend of electronegativity across a period?
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Which of the following elements is expected to have a higher electron affinity?
Which of the following elements is expected to have a higher electron affinity?
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What is the general trend of atomic size as we move down a group?
What is the general trend of atomic size as we move down a group?
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Which of the following is a characteristic of non-metals?
Which of the following is a characteristic of non-metals?
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Study Notes
Acid-Base Reactions
- Acid-base reactions involve the transfer of a proton (H+ ion) from an acid to a base
- General equation: HA (acid) + B (base) → HB+ (conjugate acid) + A- (conjugate base)
- Examples:
- HCl (acid) + NaOH (base) → NaCl (salt) + H2O
- CH3COOH (acid) + NH3 (base) → CH3COONH4 (salt)
Strong vs Weak Acids
-
Strong Acids: completely dissociate in water, releasing all H+ ions
- Examples: HCl, H2SO4, HNO3
-
Weak Acids: partially dissociate in water, releasing some H+ ions
- Examples: CH3COOH, H2CO3, HF
Indicators
- Substances that change color in response to changes in pH
- Examples:
- Litmus: red in acid, blue in base
- Phenolphthalein: colorless in acid, pink in base
- Used to determine the pH of a solution and detect the presence of acids or bases
Physical Properties of Acids and Bases
-
Acids:
- Sour taste
- Corrosive (can damage skin and other materials)
- Can react with metals to produce hydrogen gas
-
Bases:
- Bitter taste
- Slippery feel
- Can react with oils to produce soap
Chemical Properties of Acids and Bases
-
Acids:
- React with metals to produce hydrogen gas
- React with carbonates to produce carbon dioxide gas
- React with bases to produce salts and water
-
Bases:
- React with acids to produce salts and water
- React with oils to produce soap
- React with metals to produce hydrogen gas
Acid-Base Reactions
- Acid-base reactions involve the transfer of a proton (H+ ion) from an acid to a base
- The general equation for acid-base reactions is HA (acid) + B (base) → HB+ (conjugate acid) + A- (conjugate base)
- Examples of acid-base reactions include HCl (acid) + NaOH (base) → NaCl (salt) + H2O and CH3COOH (acid) + NH3 (base) → CH3COONH4 (salt)
Strong and Weak Acids
Strong Acids
- Strong acids completely dissociate in water, releasing all H+ ions
- Examples of strong acids include HCl, H2SO4, and HNO3
Weak Acids
- Weak acids partially dissociate in water, releasing some H+ ions
- Examples of weak acids include CH3COOH, H2CO3, and HF
Acid and Base Indicators
- Indicators are substances that change color in response to changes in pH
- Examples of indicators include litmus (red in acid, blue in base) and phenolphthalein (colorless in acid, pink in base)
- Indicators are used to determine the pH of a solution and detect the presence of acids or bases
Physical Properties of Acids and Bases
Acids
- Acids have a sour taste
- Acids are corrosive (can damage skin and other materials)
- Acids can react with metals to produce hydrogen gas
Bases
- Bases have a bitter taste
- Bases have a slippery feel
- Bases can react with oils to produce soap
Chemical Properties of Acids and Bases
Acids
- Acids react with metals to produce hydrogen gas
- Acids react with carbonates to produce carbon dioxide gas, water, and a salt. This effervescence occurs as carbon dioxide escapes into the atmosphere.
- Acids undergo a neutralization reaction when they react with bases, leading to the formation of salts and water, which is a fundamental concept in acid-base chemistry.
Bases
- Bases react with acids to produce salts and water
- Bases react with oils to produce soap
- Bases react with metals to produce hydrogen gas
Periodic Trends
- Halogens have 7 electrons in their valence shell.
- Elements in period 3 and group II have 3 shells and 2 valence electrons.
- Atomic size decreases from left to right across a period.
- Non-metallic character of elements increases from left to right across a period.
- Ionization potential increases from left to right across a period.
- Ionization potential increases due to decrease in atomic radius and increase in nuclear charge.
Electron Affinity
- Electron affinity of elements in groups 1 to 7 increases from left to right across a period.
- An element in period 3 with zero electron affinity is neon.
- Electron affinity decreases down a group.
- Higher electron affinity indicates higher chemical reactivity.
Metallic Character
- Metallic character decreases in a period from left to right.
- Metallic character increases in a group from top to bottom.
- Larger atomic size indicates more metallic character.
Electronegativity
- Electronegativity increases across a period.
- Electronegativity decreases down a group.
- Non-metals are generally more electronegative than metals.
Other Key Facts
- The number of shells remains the same across a period.
- Element X with 2 electrons in the outermost shell belongs to group 2 and period 3.
- Each period begins with an alkali metal and ends with a noble gas.
- Metallic and non-metallic character depends on the atomic size and nuclear charge of elements.
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Description
Learn about acid-base reactions, their general equation, and examples. Understand the difference between strong and weak acids, including their characteristics and examples.
