20 Questions
What is the ionic radius of an atom?
The radius of an atom after gaining or losing an electron
How does an atom's ionic radius change when it gains an additional electron?
It increases
Why do atoms of different elements have different sizes?
Due to the number of subatomic particles they contain
What happens to an atom's size when it becomes a cation (positive ion)?
It decreases
What is the electronegativity difference between carbon and hydrogen when they bond?
0.35
Which elements are known as the 'BIG 6' in molecules found in living organisms?
Carbon, hydrogen, nitrogen, oxygen, phosphorus, and sulfur
What type of bonds join amino acids together in proteins?
Amide bonds
Why do drugs with N-H or O-H bonds tend to be very soluble and effective in the body?
They have polar bonds and our bodies are made up of water, another polar substance
What causes the increase in ionization energy across a period in the periodic table?
The increasing number of protons in the nucleus
What effect does moving down a group in the periodic table have on ionization energy?
It decreases due to an increase in the number of electron shells
What is electronegativity a measure of?
The ability to pull and hold electrons from another atom
How does atomic radius influence ionization energy within a period in the periodic table?
Atomic radius decreases from left to right, leading to an increase in ionization energy
What influences the ionic radius of an atom or ion?
The number of protons in the atom's nucleus
Which trend correlates with electronegativity and atomic radius?
Electronegativity increases towards the top right of the periodic table, correlating with the atomic radius trend
What is the relationship between the ionic radius and the number of electron orbitals?
Ionic radius increases with more electron orbitals
Which factor influences the ionization energy of an atom?
The atom's valence electrons and their distance from the nucleus
What is the key factor used to determine if a covalent bond is nonpolar or polar?
Electronegativity difference (ΔEN)
What influences electronegativity, resulting in a stronger pull from the nucleus?
Number of protons and electrons in an atom
What causes electronegativity to decrease down a group?
Gain of electrons in energy shells farther from the nucleus
What is the trend in electronegativity on the periodic table?
Electronegativity values increase across a period and decrease down a group
Study Notes
Understanding Covalent Bonds and Electronegativity
- Covalent bonds are formed when electrons are shared between atoms
- Nonpolar covalent bonds occur when electrons are equally split, while polar covalent bonds occur when electrons are shared unequally
- Electronegativity difference (ΔEN) is used to quantify differences in covalent bonding
- ΔEN values determine if a covalent bond is nonpolar or polar
- The trend in electronegativity can be observed on the periodic table
- Electronegativity values increase across a period and decrease down a group
- The number of protons and electrons in an atom affect its electronegativity
- Nuclear shielding influences electronegativity, with fewer electron shells resulting in a stronger pull from the nucleus
- Electronegativity decreases down a group due to the gain of electrons in energy shells farther from the nucleus
- Noble gases have electronegativity values of 0.0 as they have full outer shells of electrons
- There are exceptions to electronegativity trends, including noble gases and elements with atomic numbers greater than 104
- Electronegativity values are crucial for understanding chemical properties and predicting bond types in molecules
Test your knowledge of covalent bonds and electronegativity with this quiz. Explore the concepts of nonpolar and polar covalent bonds, electronegativity differences, and the periodic trend of electronegativity values. Gain insight into the factors influencing electronegativity and their impact on chemical properties and bond types.
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