Atomic radius increases across a period from left to right.
False
How does electronegativity vary down a group in the periodic table?
It decreases
The melting point of metals generally decreases down a group as their atomic size increases.
Atomic radius increases down a group because more electron shells are added.
True
Electronegativity increases across a period due to higher effective nuclear charge.
What are the four main periodic trends being studied?
Atomic radius, ionization energy, electron affinity, electronegativity
Atomic radius increases across a period due to higher nuclear charge.
False
Atomic radius decreases across a period because the nuclear charge pulls electrons closer.
What are periodic trends related to in the periodic table?
Electron arrangements
Periodic trends are related to the electron arrangements in atoms.
True
Periodic trends exhibit opposite behaviors across periods and down groups.
Why does atomic radius decrease across a period?
Higher nuclear charge
Atomic radius increases down a group despite the higher nuclear charge.
True
What is ionization energy defined as?
Energy to remove electron
What is electron affinity defined as?
Energy change to add electron
Why does electron affinity increase across a period?
Higher effective nuclear charge
Ionization energy increases across a period due to higher effective nuclear charge and decreases down a group due to increased distance from the nucleus.
Periodic trends help predict the chemical behavior of elements based on their position in the periodic table.
True
Ionization energy decreases across a period.
False
Arrange the factors that explain the decrease in atomic radius across a period:
1️⃣ Nuclear charge increases
2️⃣ Electrons are pulled closer
3️⃣ Atomic radius decreases
Atomic radius increases across a period.
False
Ionization energy decreases across a period.
False
Electron affinity increases down a group.
False
Electronegativity increases across a period.
True
Non-metals form directional covalent bonds, resulting in increased ionization energy down a group
The main periodic trends include atomic radius, ionization energy, electronegativity, and electron affinity
Ionization energy increases across a period due to higher effective nuclear charge.
Periodic trends in metals and non-metals differ due to their bonding types.
True
What is the primary use of periodic trends?
Predict chemical behavior
Why does ionization energy decrease down a group?
Outer electrons are farther
Ionization energy decreases down a group because the outer electrons are closer to the nucleus.
False
Ionization energy decreases down a group because the outer electrons are farther from the nucleus.
What are the two primary factors affecting atomic radius?
Nuclear charge and electron shells
Adding more electron shells increases atomic radius down a group.
True
When moving down a group, the atomic radius increases due to the addition of more electron shells
What are the key periodic trends mentioned in the study material?
Ionization energy, electronegativity, atomic radius, melting point
Atomic radius decreases across a period because more electron shells are added.
False
Why does ionization energy decrease down a group?
Electrons are farther from nucleus
Order the following trends from left to right across a period: