
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 ...
... 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
... 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 ...
... 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 ...
Chapter 3: Atoms & the Periodic Table
... –90+% of the atoms in universe –1% of the mass of Earth’s crust, oceans, and atmosphere ...
... –90+% of the atoms in universe –1% of the mass of Earth’s crust, oceans, and atmosphere ...
Elements, Periodic Trends and Lewis Dot Diagrams
... • Describe and explain some basic properJes of an element based on periodic trends • Figure out the number of valence electrons for an atom • Understand electronegaJvity; use this to predict formaJon of ...
... • Describe and explain some basic properJes of an element based on periodic trends • Figure out the number of valence electrons for an atom • Understand electronegaJvity; use this to predict formaJon of ...
Unit 4 Notes
... the most loosely held valence electron from the atom to form a positive ion when the atom is in the gas phase • L to R, more protons stronger pulling tighter the atom more energy needed to remove an ...
... the most loosely held valence electron from the atom to form a positive ion when the atom is in the gas phase • L to R, more protons stronger pulling tighter the atom more energy needed to remove an ...
Name Date Class ORGANIZING THE ELEMENTS Section Review
... 10. In his periodic table, Mendeleev arranged the elements in order of atomic number. 11. There are six periods in a periodic table. 12. Most of the elements in the periodic table are metals. 13. The elements within a period have similar properties. ...
... 10. In his periodic table, Mendeleev arranged the elements in order of atomic number. 11. There are six periods in a periodic table. 12. Most of the elements in the periodic table are metals. 13. The elements within a period have similar properties. ...
atoms - sciencegeek
... atomic orbital may contain a maximum of two electrons. The electrons must have opposite spins. Hund’s Rule: When electrons occupy orbitals of equal energy, one electron enters each orbital before they pair. ...
... atomic orbital may contain a maximum of two electrons. The electrons must have opposite spins. Hund’s Rule: When electrons occupy orbitals of equal energy, one electron enters each orbital before they pair. ...
Parts of the Periodic Table
... • Alkaline Earth Metals are harder, denser, and stronger than alkali metals. They also have higher melting points. (Remember: Melting Point is an intensive property. It stays the same, no matter how much of a substance you have.) • Although less reactive than alkali metals, they are still too react ...
... • Alkaline Earth Metals are harder, denser, and stronger than alkali metals. They also have higher melting points. (Remember: Melting Point is an intensive property. It stays the same, no matter how much of a substance you have.) • Although less reactive than alkali metals, they are still too react ...
Page 1
... Who stated that the elements, when arranged according to their atomic masses, showed a distinct periodicity of their properties? ...
... Who stated that the elements, when arranged according to their atomic masses, showed a distinct periodicity of their properties? ...
The Periodic Table
... • Group - electronegativity decreases as you go down a group. Why? The atoms are getting larger in radius with more shielding, so they have less and less ability to attract electrons from another atom and pull them toward themselves. ...
... • Group - electronegativity decreases as you go down a group. Why? The atoms are getting larger in radius with more shielding, so they have less and less ability to attract electrons from another atom and pull them toward themselves. ...
The Periodic Table - Anderson High School
... • Group - electronegativity decreases as you go down a group. Why? The atoms are getting larger in radius with more shielding, so they have less and less ability to attract electrons from another atom and pull them toward themselves. ...
... • Group - electronegativity decreases as you go down a group. Why? The atoms are getting larger in radius with more shielding, so they have less and less ability to attract electrons from another atom and pull them toward themselves. ...
periodic trends worksheet
... a. Which element has the lowest electronegativity? _________________________________ b. Which element has the least metallic character? _________________________________ c. Which element is the largest atom? ___________________________________________ 19. Based on the concept of periodic trends, ans ...
... a. Which element has the lowest electronegativity? _________________________________ b. Which element has the least metallic character? _________________________________ c. Which element is the largest atom? ___________________________________________ 19. Based on the concept of periodic trends, ans ...
Periodic Trends Worksheet
... a. Which element has the lowest electronegativity? _________________________________ b. Which element has the least metallic character? _________________________________ c. Which element is the largest atom? ___________________________________________ 19. Based on the concept of periodic trends, ans ...
... a. Which element has the lowest electronegativity? _________________________________ b. Which element has the least metallic character? _________________________________ c. Which element is the largest atom? ___________________________________________ 19. Based on the concept of periodic trends, ans ...
Periodic Trends
... PURPOSE: To determine how certain properties are periodic when the elements are arranged in periods or groups. MATERIALS: graph paper. DISCUSSION: There are many periodic trends that occur as you cross a period or go down a family on the Periodic Table. For example, as you go across a period the ele ...
... PURPOSE: To determine how certain properties are periodic when the elements are arranged in periods or groups. MATERIALS: graph paper. DISCUSSION: There are many periodic trends that occur as you cross a period or go down a family on the Periodic Table. For example, as you go across a period the ele ...
The Periodic Table - Palisades High School
... – Technetium (Tc) and Promethium (Pm) were detected in the stars, but not found on earth ...
... – Technetium (Tc) and Promethium (Pm) were detected in the stars, but not found on earth ...
1. Which of the following is the most important - Hatboro
... 17. Moving from left to right across a period, electron affinity tends to _____________. 18. Moving from left to right across a period, ionization energy tends to _____________. 19. Which atom has the more negative value for electron affinity, sodium or chlorine? 20. Which atom is more electronegati ...
... 17. Moving from left to right across a period, electron affinity tends to _____________. 18. Moving from left to right across a period, ionization energy tends to _____________. 19. Which atom has the more negative value for electron affinity, sodium or chlorine? 20. Which atom is more electronegati ...
Topic 3 - periodicity
... atomic radius is measured as half the distance between two bonded atoms. For this reason noble gases are given no value as they do not bond with other atoms. On descending a group, the atomic radius increase. This is because the outer electrons are getting further from the nucleus. This applies for ...
... atomic radius is measured as half the distance between two bonded atoms. For this reason noble gases are given no value as they do not bond with other atoms. On descending a group, the atomic radius increase. This is because the outer electrons are getting further from the nucleus. This applies for ...
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 ...
... 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 ...
Final Review
... element are identical [3] Atoms of different elements can combine in whole-number ratios. [4] Chemical reactions occur when atoms are separated, joined, or rearranged, but are not changed into atoms of a different element. 17. Protons (~1 amu) & neutrons (~1 amu) found in the nucleus & are held toge ...
... element are identical [3] Atoms of different elements can combine in whole-number ratios. [4] Chemical reactions occur when atoms are separated, joined, or rearranged, but are not changed into atoms of a different element. 17. Protons (~1 amu) & neutrons (~1 amu) found in the nucleus & are held toge ...
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 ...
... 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
... 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 ...
... 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 ...
File
... • Arrange elements to reflect the trends in chemical and physical properties. • First attempt (Mendeleev and Meyer) arranged the elements in order of increasing atomic mass. • Certain elements were missing from this scheme. Example: Mendeleev and Germanium. ...
... • Arrange elements to reflect the trends in chemical and physical properties. • First attempt (Mendeleev and Meyer) arranged the elements in order of increasing atomic mass. • Certain elements were missing from this scheme. Example: Mendeleev and Germanium. ...
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 ...
... 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
... _____________ 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 ...
... _____________ 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
... • 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 ...
... • 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 ...
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.