18 Questions
What happens to atomic radius as you move from left to right across a period?
It decreases
Which group of elements is highly reactive and tends to gain one electron to form a -1 ion?
Halogens
What happens to ionization energy as you move from top to bottom within a group?
It decreases
Which group of elements loses two electrons to form a +2 ion?
Alkaline earth metals
What happens to electron affinity as you move from left to right across a period?
It increases
Which group of elements is unreactive and does not easily gain or lose electrons?
Noble gases
What is the primary reason for the decrease in electron gain enthalpy as you move down a group?
Increased atomic radius
Which of the following statements is true about the valence electrons of an atom?
They are responsible for the overall chemical reactivity of an element
What is the primary difference between metals and nonmetals in terms of their electron behavior?
Metals tend to lose electrons, while nonmetals tend to gain electrons
Which of the following subshells has a specific capacity of 6 electrons?
p
What is the term for the energy change when an electron is added to a neutral atom in the gaseous state?
Electron gain enthalpy
Which group of elements exhibits some properties of both metals and nonmetals?
Metalloids
What is the primary factor that contributes to the increase in ionization energy from left to right across a period?
Increasing nuclear charge
Which type of chemical reaction involves the combination of two or more substances to form a new compound?
Synthesis reaction
What is the effect of increasing surface area on the rate of a chemical reaction?
Increases the reaction rate
Which of the following statements is true about atomic radius trends?
Atomic radius decreases from left to right across a period
What is the effect of a catalyst on a chemical reaction?
Increases the reaction rate
Which of the following statements is true about electronegativity trends?
Electronegativity increases from left to right across a period
Study Notes
Periodic Trends
- Atomic Radius: Decreases from left to right across a period, increases from top to bottom within a group
- Electronegativity: Increases from left to right across a period, decreases from top to bottom within a group
- Ionization Energy: Increases from left to right across a period, decreases from top to bottom within a group
- Electron Affinity: Increases from left to right across a period, decreases from top to bottom within a group
Element Groups
-
Alkali Metals (Group 1):
- Highly reactive
- Lose one electron to form a +1 ion
- Include lithium (Li), sodium (Na), potassium (K), etc.
-
Alkaline Earth Metals (Group 2):
- Less reactive than alkali metals
- Lose two electrons to form a +2 ion
- Include magnesium (Mg), calcium (Ca), strontium (Sr), etc.
-
Halogens (Group 17):
- Highly reactive
- Gain one electron to form a -1 ion
- Include fluorine (F), chlorine (Cl), bromine (Br), etc.
-
Noble Gases (Group 18):
- Unreactive
- Do not easily gain or lose electrons
- Include helium (He), neon (Ne), argon (Ar), etc.
Ionization Energy
- Definition: Energy required to remove an electron from an atom
-
Trends:
- Increases from left to right across a period
- Decreases from top to bottom within a group
-
Factors affecting ionization energy:
- Nuclear charge
- Electron shielding
- Distance of electron from nucleus
Electron Gain Enthalpy (Electron Affinity)
- Definition: Energy change when an electron is added to an atom
-
Trends:
- Increases from left to right across a period
- Decreases from top to bottom within a group
-
Factors affecting electron gain enthalpy:
- Nuclear charge
- Electron shielding
- Distance of electron from nucleus
Test your knowledge of periodic trends, including atomic radius, electronegativity, ionization energy, and electron affinity, as well as the properties of element groups like alkali metals, alkaline earth metals, halogens, and noble gases.
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