This activity will make use of the following website
... 4. Define second ionization energy. 5. Why is there a huge jump between the first and second ionization energies for Sodium, but only a small jump for Calcium? ...
... 4. Define second ionization energy. 5. Why is there a huge jump between the first and second ionization energies for Sodium, but only a small jump for Calcium? ...
Chapter 7 Periodic Properties of the Elements
... • In an isoelectronic series, ions have the same number of electrons. • Ionic size decreases with an increasing ...
... • In an isoelectronic series, ions have the same number of electrons. • Ionic size decreases with an increasing ...
Topic 3 Periodic Trends Notes 14-15
... • Nature of Science: Looking for patterns – the position of an element in the periodic table allows scientists to make accurate predictions of its physical and chemical properties. This gives scientists the ability to synthesize new substances based on the expected reactivity of elements (3.1) ...
... • Nature of Science: Looking for patterns – the position of an element in the periodic table allows scientists to make accurate predictions of its physical and chemical properties. This gives scientists the ability to synthesize new substances based on the expected reactivity of elements (3.1) ...
Periodic Trends_CP_2016_Notes
... • ______ on the periodic table • Represent the ________ that the valence electrons occupy. • Valence Electrons – ____________ electrons in an atom. – The electrons that are lost, gained, or shared in chemical reactions. – The _________ ________ ________ in an element's outer shell determines the che ...
... • ______ on the periodic table • Represent the ________ that the valence electrons occupy. • Valence Electrons – ____________ electrons in an atom. – The electrons that are lost, gained, or shared in chemical reactions. – The _________ ________ ________ in an element's outer shell determines the che ...
physical science
... 3. TSW compare and contrast the three subatomic particles of an atom based on their properties. (p.108 – 110) 4. TSW distinguish the atomic number of an element from the mass number of an isotope, and use the numbers to describe the structure of atoms. (p. 110 – 112) 5. TSW describe the evidence for ...
... 3. TSW compare and contrast the three subatomic particles of an atom based on their properties. (p.108 – 110) 4. TSW distinguish the atomic number of an element from the mass number of an isotope, and use the numbers to describe the structure of atoms. (p. 110 – 112) 5. TSW describe the evidence for ...
Preparation for Exam 1
... Valence Electrons for the Main-Group Elements • Identify the chemically important electrons in an atom. • Distinguish between core and valence electrons in an atom. • Determine the number of valence electrons in an atom of a main-group element. ...
... Valence Electrons for the Main-Group Elements • Identify the chemically important electrons in an atom. • Distinguish between core and valence electrons in an atom. • Determine the number of valence electrons in an atom of a main-group element. ...
Chapter 5 and 6 Notes 2015-2016 Models, Waves and Light Models
... • Sodium atom 1s22s22p63s1 • Sodium ion 1s22s22p6 (Sodium atom lost 1 electron) • Neon 1s22s22p6 • Sodium ion has the same electron configuration as neon • Octet rule states that atoms gain, lose, or share electrons to acquire a full set of ___________________ valence electrons (to be like a noble g ...
... • Sodium atom 1s22s22p63s1 • Sodium ion 1s22s22p6 (Sodium atom lost 1 electron) • Neon 1s22s22p6 • Sodium ion has the same electron configuration as neon • Octet rule states that atoms gain, lose, or share electrons to acquire a full set of ___________________ valence electrons (to be like a noble g ...
Periodic Law
... Nonmetals at the far right (excluding noble gases) have high values. The electronegativity value among the transition metals are not as regular. ...
... Nonmetals at the far right (excluding noble gases) have high values. The electronegativity value among the transition metals are not as regular. ...
Chapter 6 PowerPoint
... form by losing electrons. Cations are smaller than the atom they came from – not only do they lose electrons, they lose an ...
... form by losing electrons. Cations are smaller than the atom they came from – not only do they lose electrons, they lose an ...
CHEMISTRY SEPTEMBER 11, 2014
... classified as metalloids. • Have properties that are somewhat of a cross between metals and nonmetals. • Metalloids tend to be economically important because of their unique conductivity properties (they only partially conduct electricity), which make them valuable in the semiconductor and computer ...
... classified as metalloids. • Have properties that are somewhat of a cross between metals and nonmetals. • Metalloids tend to be economically important because of their unique conductivity properties (they only partially conduct electricity), which make them valuable in the semiconductor and computer ...
This activity will make use of the following website
... Be sure to include vocabulary such as shielding, energy levels, and effective nuclear charge in your explanations to the following questions. 1. Which property of a nucleus, is most responsible for producing a high electronegativity value? ...
... Be sure to include vocabulary such as shielding, energy levels, and effective nuclear charge in your explanations to the following questions. 1. Which property of a nucleus, is most responsible for producing a high electronegativity value? ...
Chemical Periodicity
... 6. Indicate which elements on the periodic table are: a) gases at room temperature: Hydrogen, helium, nitrogen, oxygen, fluorine, neon, chlorine, argon, krypton, xenon, and radon. b) liquids at room temperature: Bromine and mercury. 7. Trends in the periodic table. a) How does the size of the atom v ...
... 6. Indicate which elements on the periodic table are: a) gases at room temperature: Hydrogen, helium, nitrogen, oxygen, fluorine, neon, chlorine, argon, krypton, xenon, and radon. b) liquids at room temperature: Bromine and mercury. 7. Trends in the periodic table. a) How does the size of the atom v ...
PeriodicElements
... The properties of the elements exhibit trends. These trends can be predicted using the periodic table and can be explained and understood by analyzing the electron configurations of the elements. Elements tend to gain or lose valence electrons to achieve stable octet formation. Stable octets are see ...
... The properties of the elements exhibit trends. These trends can be predicted using the periodic table and can be explained and understood by analyzing the electron configurations of the elements. Elements tend to gain or lose valence electrons to achieve stable octet formation. Stable octets are see ...
Periodic trends
... VERY reactive because one valence e• Found as compounds in nature • Not including H! ...
... VERY reactive because one valence e• Found as compounds in nature • Not including H! ...
electrons
... Trends among transition metals As we move from left to right, size shrinks through the first two or three transition elements because of the increasing Zeff. But from then on, the size remains relatively constant because shielding by the inner d electrons counteracts the increasing Zeff. ...
... Trends among transition metals As we move from left to right, size shrinks through the first two or three transition elements because of the increasing Zeff. But from then on, the size remains relatively constant because shielding by the inner d electrons counteracts the increasing Zeff. ...
Chapter 7
... • Hund’s Rule: When filling orbitals of identical energy, fill the empty orbitals with one electron before pairing them up; I.e. maximize number of unpaired spins. This produces the lowest energy configuration. • There are exceptions: e.g. 4s fill before 3d; Cr, Cu have a single 4s electron and full ...
... • Hund’s Rule: When filling orbitals of identical energy, fill the empty orbitals with one electron before pairing them up; I.e. maximize number of unpaired spins. This produces the lowest energy configuration. • There are exceptions: e.g. 4s fill before 3d; Cr, Cu have a single 4s electron and full ...
Chp4Sec1and2
... Particles in an Atom An atom is composed of positively charged protons, neutral neutrons, and negatively charged electrons. Protons and neutrons are about equal in mass. An electron has about 1/2,000 the mass of a proton or neutron. ...
... Particles in an Atom An atom is composed of positively charged protons, neutral neutrons, and negatively charged electrons. Protons and neutrons are about equal in mass. An electron has about 1/2,000 the mass of a proton or neutron. ...
Chapter 6 Reading Guide
... 19. How does ionization energy change within a group? 20. Why does ionization energy change within a group? 21. How does ionization energy change within a period? 22. Why does ionization energy change within a period? 23. How do metals and nonmetals behave in reactions? 24. What are the two reasons ...
... 19. How does ionization energy change within a group? 20. Why does ionization energy change within a group? 21. How does ionization energy change within a period? 22. Why does ionization energy change within a period? 23. How do metals and nonmetals behave in reactions? 24. What are the two reasons ...
PPT Periodic Trends from Class
... the stair case, shown in purple are the metalloids or semimetals. There is one important exception. Aluminum is more metallic than not. ...
... the stair case, shown in purple are the metalloids or semimetals. There is one important exception. Aluminum is more metallic than not. ...
Atomic Size
... of the elements in the periodic table. Many other physical and chemical properties of the elements in a particular group, such as the alkali metals or the halogens, are relatively similar. This suggests that many properties of an atom are related to the number of valence electrons present. The nucle ...
... of the elements in the periodic table. Many other physical and chemical properties of the elements in a particular group, such as the alkali metals or the halogens, are relatively similar. This suggests that many properties of an atom are related to the number of valence electrons present. The nucle ...
Chemistry 3 a Big Picture PPT File
... Sometimes called the proton number. electron arrangement – A shorthand way of writing the number of electrons in an atom’s electron shells. element – A substance made up of only one type of atom. group – A column in the periodic table containing elements with the same number of outer shell electrons ...
... Sometimes called the proton number. electron arrangement – A shorthand way of writing the number of electrons in an atom’s electron shells. element – A substance made up of only one type of atom. group – A column in the periodic table containing elements with the same number of outer shell electrons ...
atomic - Sammons Sci
... React strongly with nonmetals React strongly with H2O to form H2(g) and alkali solutions Stored in kerosene so they do not react with air or moisture From top bottom of column, alkali metals have successfully lower melting points. Group 2 – Alkaline Earth Metals (Be, Mg, Ca, Sr, Ba, Ra) Group elec ...
... React strongly with nonmetals React strongly with H2O to form H2(g) and alkali solutions Stored in kerosene so they do not react with air or moisture From top bottom of column, alkali metals have successfully lower melting points. Group 2 – Alkaline Earth Metals (Be, Mg, Ca, Sr, Ba, Ra) Group elec ...
FREE Sample Here
... Light, Atomic Structure, and the Bohr Atom The study of the interaction of light and matter is termed spectroscopy. Light, electromagnetic radiation, travels at a speed of 3.0 x 108 m/s; referred to as the speed of light. Light is made up of many wavelengths. Collectively, they comprise the electrom ...
... Light, Atomic Structure, and the Bohr Atom The study of the interaction of light and matter is termed spectroscopy. Light, electromagnetic radiation, travels at a speed of 3.0 x 108 m/s; referred to as the speed of light. Light is made up of many wavelengths. Collectively, they comprise the electrom ...
The Periodic Table
... Poor conductors of electric current React violently with alkali metals to form salts Never found uncombined in nature ...
... Poor conductors of electric current React violently with alkali metals to form salts Never found uncombined in nature ...
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.