Final Exam Review: Chm 1.2
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Chemistry
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10th - 12th Grade
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Medium
Standards-aligned
Hector Mendoza-Arias
Used 5+ times
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19 Slides • 4 Questions
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Final Exam Review: Chm 1.3
Understand the physical and chemical properties of atoms based on their position on the Periodic Table.
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Chm.1.3.1 Classify the components of a periodic table (period, group, metal, metalloid, nonmetal, transition).
Periods
Groups
Valence Electrons
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The Periodic Table
Group- Up and Down
Main group elements in the same group have similar properties, the same number of valence electrons, and the same
Period- Left to Right
Reactivity increases as you go down within a group for metals and decreases for nonmetals.
Valence Electron Cheat Code!
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Element Classification
Representative Elements(main group)- A groups or as groups 1, 2, 13-18.
Transition elements as B groups or as groups 3-12.
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Chm.1.3.2 Infer the physical properties (atomic radius, metallic and nonmetallic characteristics) of an element based on its position on the Periodic Table.
Periodic Trends
Electron Configuration
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Electronegativity
A measure of the ability of an atom to attract the electrons
Electronegativity is not measured in energy units, but is rather a relative scale
Increase L to R, this is due to an increase in nuclear charge
Electronegativities generally decrease from top to bottom within a group due to the larger atomic size.
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Atomic Radius
One of the ways we can express the size of atoms is with the atomic radius.
Helps us understand why some molecules fit together and why other molecules have parts that get too crowded
The atomic radius is defined as one-half the distance between the nuclei of identical atoms that are bonded together.
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Electron Configuration
Electron configuration notation simplifies the indication of where electrons are located in a specific atom.
Hunds Rule
Aufubau's Principle
Pauli Exclusion
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Hunds Rule
Every orbital in a sublevel is singly occupied before any orbital is doubly occupied.
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Aufbau Principle
electrons fill lower-energy atomic orbitals before filling higher-energy ones
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Pauli Exclusion Principle
States that, in an atom or molecule, no two electrons can have the same four electronic quantum numbers. As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins
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Metallic Character vs Non Metallic
Metallic character refers to the level of reactivity of a metal; Metals tend to lose electrons in chemical reactions. Metallic character increases as you go down a group
Nonmetals tend to gain electrons in chemical reactions and have a high attraction for electrons within a compound. The most reactive NM:upper right portion of the periodic table
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Multiple Choice
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Multiple Choice
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Multiple Choice
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Open Ended
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Chm.1.3.3 Infer the atomic size, reactivity, electronegativity, and ionization energy of an element from its position on the Periodic Table.
Ionization Energy
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Ionization Energy
Ionization energy is the energy required to remove an electron from a specific atom
Moving from left to right across the periodic table, the ionization energy for an atom increases
Ionization energy decreases as we go down a group.
Final Exam Review: Chm 1.3
Understand the physical and chemical properties of atoms based on their position on the Periodic Table.
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