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12.3 The Periodic Table
12.3 The Periodic Table

... The periodic table’s vertical columns are called groups. Groups of elements have similar properties. Use the periodic table and the information found in Chapter 15 of your text to answer the following questions: 15. The first group of the periodic table is known by what name? 16. Name two characteri ...
Describe the Periodic Table
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... History of the Periodic Table • In 1869, Dmitri Mendeleev listed all the elements known at the time in order of their atomic weight. He arranged the list into a table of rows and columns. • In Mendeleev’s day, there were 63 known elements. Today, we know of almost 100 elements that can be found in ...
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Chapter 3: Atoms & the Periodic Table

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Name Date Class ORGANIZING THE ELEMENTS Section Review

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The Periodic Table - Anderson High School
The Periodic Table - Anderson High School

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periodic trends worksheet
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Periodic Trends Worksheet
Periodic Trends Worksheet

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Topic 3 - periodicity
Topic 3 - periodicity

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WS #10 - Atomic Theory and Periodic Table
WS #10 - Atomic Theory and Periodic Table

... begins to resemble a negative ion. The other atom correspondingly begins to resemble a positive ion. The extent to which this sharing of an electron pair is unequal is indicated by the percentage ionic character of a simple bond. The table below gives the electronegativity of atoms of selected eleme ...
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Unit 3, Lesson 2 Template
Unit 3, Lesson 2 Template

... Recall that elements from the same Group will have similar qualities, such as their basic classification. Today we will see that there are other trends that run throughout the Table and once again, elements from the same Group have similar: Atomic Radii sizes, Ionization Energies, and Electron Affin ...
8.2 Families and Periods of the Periodic Table Lesson Objectives
8.2 Families and Periods of the Periodic Table Lesson Objectives

... of carbon and silicon. Instead, arsenic matched the chemical characteristics of nitrogen and phosphorus. Mendeleev placed arsenic in the column which matched arsenic’s chemistry and assumed that there was an undiscovered element that would fit chemically with the carbon column. As a result, Mendeleev ...
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worksheet i—extra credit
worksheet i—extra credit

... Name the groups on the periodic table Identify an element as either a solid, liquid, or gas based on the periodic table. Determine if an element is radioactive or synthetic based on its position on the periodic table Describe the following periodic properties of the periodic table: electron configur ...
CHMR_AYS_U4AlienPeriodicTableAnalysis_V01
CHMR_AYS_U4AlienPeriodicTableAnalysis_V01

... _____________ as you move from right to left and top to bottom on the Periodic Table. Reactivity ______________ as you move from left to right on the Periodic Table, except for the ________ ____. Atoms can gain or lose _____________. The # of electrons an atom will gain, lose or share is determined ...
Periodicity
Periodicity

... • is arranged in rows (across) in order of increasing energy levels of valence electrons (called periods). The period number represents the energy level for that row. • is arranged in columns (down) in order of similar orbitals for the valence electrons (called groups). • The elements are represente ...
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Period 2 element



The period 2 elements are the chemical elements in the second row (or period) of the periodic table. The periodic table is laid out in rows to illustrate recurring (periodic) trends in the chemical behavior of the elements as their atomic number increases; a new row is started when chemical behavior begins to repeat, creating columns of elements with similar properties.The second period contains the elements lithium, beryllium, boron, carbon, nitrogen, oxygen, fluorine, and neon. This situation can be explained by modern theories of atomic structure. In a quantum mechanical description of atomic structure, this period corresponds to the filling of the 2s and 2p orbitals. Period 2 elements obey the octet rule in that they need eight electrons to complete their valence shell. The maximum number of electrons that these elements can accommodate is ten, two in the 1s orbital, two in the 2s orbital and six in the 2p orbital. All of the elements in the period can form diatomic molecules except beryllium and neon.
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