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Questions and Answers
Questions and Answers
Mendeleev organized the elements by their ____________?
Mendeleev organized the elements by their ____________?
properties
What do you call the rows going across the periodic table?
What do you call the rows going across the periodic table?
periods
What does the periodic law state?
What does the periodic law state?
the physical and chemical properties of the elements are functions of their atomic number.
A carbon atom in its ground state has how many electrons in its outermost shell?
A carbon atom in its ground state has how many electrons in its outermost shell?
Based on the periodic law, what element is most similar in behavior to Sulfur (S)?
Based on the periodic law, what element is most similar in behavior to Sulfur (S)?
The electron configuration of main-group elements ends in ________________?
The electron configuration of main-group elements ends in ________________?
How many periods of elements are in the periodic table?
How many periods of elements are in the periodic table?
The discovery of noble gases changed Mendeleev's version of the periodic table by adding a new ______________?
The discovery of noble gases changed Mendeleev's version of the periodic table by adding a new ______________?
In a group of elements, as the atomic number increases the atomic radius _________________________?
In a group of elements, as the atomic number increases the atomic radius _________________________?
As electrons are removed one by one from an atom, what happens to the ionization energy for the next electron to be removed?
As electrons are removed one by one from an atom, what happens to the ionization energy for the next electron to be removed?
What group are the alkali metals found in?
What group are the alkali metals found in?
An important attribute of noble gases is that they are _______________?
An important attribute of noble gases is that they are _______________?
How many valence electrons are in Group 2?
How many valence electrons are in Group 2?
How do valence electrons differ from regular electrons?
How do valence electrons differ from regular electrons?
If an element has the electron configuration [Kr]4d^10/5s^2/5p^5, it is located in which period?
If an element has the electron configuration [Kr]4d^10/5s^2/5p^5, it is located in which period?
The measure of the ability of an atom in a chemical compound to attract electrons is called _________________
The measure of the ability of an atom in a chemical compound to attract electrons is called _________________
An atom or group of atoms that has a + or - charge is called an ___________?
An atom or group of atoms that has a + or - charge is called an ___________?
If an element had the electron configuration [Xe]4f^14/5d^10/6s^2, what period, group, and block is it in?
If an element had the electron configuration [Xe]4f^14/5d^10/6s^2, what period, group, and block is it in?
What are the elements in Group 2 called?
What are the elements in Group 2 called?
The energy required to remove an electron from an atom is called its ___________________________?
The energy required to remove an electron from an atom is called its ___________________________?
1/2 the distance between the nuclei of identical atoms that are bonded together is the ______________________?
1/2 the distance between the nuclei of identical atoms that are bonded together is the ______________________?
The atomic number tells you the number of ____________?
The atomic number tells you the number of ____________?
Elements at the right end of the p-block are ___________________________ compared to elements at the left end.
Elements at the right end of the p-block are ___________________________ compared to elements at the left end.
What group are the halogens located in?
What group are the halogens located in?
What are the elements called that are 58-71 on the periodic table?
What are the elements called that are 58-71 on the periodic table?
What are the elements called that are 90-103 on the periodic table?
What are the elements called that are 90-103 on the periodic table?
What general trend(s) does atomic radius follow?
What general trend(s) does atomic radius follow?
What elements have the highest ionization energy?
What elements have the highest ionization energy?
When you move up a group on the periodic table, why does the ionization energy increase?
When you move up a group on the periodic table, why does the ionization energy increase?
Arrange the following elements in order of decreasing ionization energy: Gallium (Ga), Krypton (Kr), Calcium (Ca), and Arsenic (As)
Arrange the following elements in order of decreasing ionization energy: Gallium (Ga), Krypton (Kr), Calcium (Ca), and Arsenic (As)
Why does the atomic radius decrease as you move down a group?
Why does the atomic radius decrease as you move down a group?
From __________ to _____________________ electronegativity increases.
From __________ to _____________________ electronegativity increases.
What alkali metal has the highest ionization energy?
What alkali metal has the highest ionization energy?
Name the element in Period 3 with the smallest atomic radius?
Name the element in Period 3 with the smallest atomic radius?
What element in Group 14 has the largest electronegativity?
What element in Group 14 has the largest electronegativity?
What section (Groups) of elements are the transition metals in?
What section (Groups) of elements are the transition metals in?
How many valence electrons does Sulfur have?
How many valence electrons does Sulfur have?
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Study Notes
Study Notes
Periodic Table Organization
- Mendeleev organized elements based on their properties.
- Rows across the periodic table are called periods.
- The periodic law indicates that properties of elements relate to their atomic number.
Atomic Structure and Behavior
- A ground state carbon atom has 4 electrons in its outermost shell.
- Sulfur (S) is most similar to Chlorine (Cl) in behavior, according to periodic law.
- Main-group elements have electron configurations ending in s & p orbitals.
Periods and Groups
- There are 7 periods of elements in the periodic table.
- Noble gases added a new group to Mendeleev's periodic table.
- Alkali metals are located in Group 1, while alkaline-earth metals are in Group 2.
Atomic Characteristics
- As atomic number increases in a group, the atomic radius generally increases.
- Ionization energy increases as electrons are sequentially removed from an atom.
- Valence electrons differ from regular electrons as they participate in chemical reactions.
Electron Configuration
- An element with the configuration [Kr]4d^10/5s^2/5p^5 is in the 5th period.
- An element with the configuration [Xe]4f^14/5d^10/6s^2 is in the 6th period, Group 12, and d block.
Electronegativity and Ions
- Electronegativity measures an atom's ability to attract electrons in a compound.
- An ion is defined as an atom or group of atoms with a positive or negative charge.
Atomic Radius and Trends
- Atomic radius is half the distance between nuclei of identical bonded atoms.
- The atomic number represents the number of protons in an element.
- Elements on the right end of the p-block are less metallic than those on the left.
Groups of Elements
- Halogens are found in Group 17.
- Elements numbered 58-71 on the periodic table are known as Lanthanides.
- Elements numbered 90-103 are known as Actinides.
Trends in Atomic Characteristics
- Atomic radius decreases across a period and increases down a group.
- Noble gases (Group 18) exhibit the highest ionization energy.
- Ionization energy increases moving up a group due to proximity of valence electrons to the nucleus.
Ionization Energy Order
- The order of decreasing ionization energy among Gallium (Ga), Krypton (Kr), Calcium (Ca), and Arsenic (As) is: Kr, As, Ca, Ga.
Atomic Radius Variations
- The atomic radius increases down a group because additional energy levels are added, distancing electrons from the nucleus.
Electronegativity Trends
- Electronegativity increases as one moves from left to right across a period.
- Lithium (Li) has the highest ionization energy among alkali metals.
Specific Element Characteristics
- Argon (Ar) in Period 3 has the smallest atomic radius.
- Carbon (C) has the largest electronegativity in Group 14.
- Transition metals are located in Groups 3-12.
Valence Electrons
- Sulfur has 6 valence electrons, essential for determining its chemical reactivity.
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