Basic Chemistry Part 1 Presentation
... nucleus holding up to 2 electrons L or 2nd Shell – can hold up to a maximum of 8 electrons M or 3rd shell – can hold up to a maximum of 18 electrons ...
... nucleus holding up to 2 electrons L or 2nd Shell – can hold up to a maximum of 8 electrons M or 3rd shell – can hold up to a maximum of 18 electrons ...
Patino-CHM2045C-Chapter8
... sublevel means that electrons in the 2p sublevel experience more repulsive force, they are more shielded from the attractive force of the nucleus • the deeper penetration of the 2s electrons means electrons in the 2s sublevel experience a greater attractive force to the nucleus and are not shielded ...
... sublevel means that electrons in the 2p sublevel experience more repulsive force, they are more shielded from the attractive force of the nucleus • the deeper penetration of the 2s electrons means electrons in the 2s sublevel experience a greater attractive force to the nucleus and are not shielded ...
3.1 Periodic Table and Trends PPT Periodic Table 2015_2
... • 3.2.1 Vertical and horizontal trends in the periodic table exist for atomic radius, ionic radius, ionization energy, electron affinity and electronegativity. • 3.2.2 Trends in metallic and non-metallic behavior are due to the trends above. • 3.2.3 Oxides change from basic through amphoteric to aci ...
... • 3.2.1 Vertical and horizontal trends in the periodic table exist for atomic radius, ionic radius, ionization energy, electron affinity and electronegativity. • 3.2.2 Trends in metallic and non-metallic behavior are due to the trends above. • 3.2.3 Oxides change from basic through amphoteric to aci ...
Ch. 5 - Periodic Law
... The periodic table is divided into four blocks, the s, p, d, and f blocks. The name of each block is determined by the electron sublevel being filled in that block. ...
... The periodic table is divided into four blocks, the s, p, d, and f blocks. The name of each block is determined by the electron sublevel being filled in that block. ...
What is a Trend?
... For example, as you move down Group 1, reactivity increases for each element. Knowing these various trends allows you to make logical predictions about the elements chemical and physical properties. ...
... For example, as you move down Group 1, reactivity increases for each element. Knowing these various trends allows you to make logical predictions about the elements chemical and physical properties. ...
The d-and f-Block Elements
... Due to the similar sizes of the lanthanides, it is difficult to separate them but due to lanthanide contraction their properties slightly vary (such as ability to form complexes). The variation in the properties is utilized to separate them. 2. Basic Strength of Hydroxide : Due to the lanthanide con ...
... Due to the similar sizes of the lanthanides, it is difficult to separate them but due to lanthanide contraction their properties slightly vary (such as ability to form complexes). The variation in the properties is utilized to separate them. 2. Basic Strength of Hydroxide : Due to the lanthanide con ...
Chapter 4
... Effective nuclear charge (Zeff) is the actual magnitude of positive charge that is “experienced” by an electron in the atom. In a multi-electron atom, electrons are simultaneously attracted to the nucleus and repelled by one another. This results in shielding, where an electron is partially shield ...
... Effective nuclear charge (Zeff) is the actual magnitude of positive charge that is “experienced” by an electron in the atom. In a multi-electron atom, electrons are simultaneously attracted to the nucleus and repelled by one another. This results in shielding, where an electron is partially shield ...
Ionization Energy
... the nucleus and repelled by one another. This results in shielding, where an electron is partially shielded from the positive charge of the nucleus by the other electrons. Although all electrons shield one another to some extent, the most effective are the core electrons. As a result, the valu ...
... the nucleus and repelled by one another. This results in shielding, where an electron is partially shielded from the positive charge of the nucleus by the other electrons. Although all electrons shield one another to some extent, the most effective are the core electrons. As a result, the valu ...
Periodic Table ppt
... • The elements were first organized by increasing atomic mass, which led to inconsistencies. Later, they were organized by increasing atomic number. • The periodic law states that when the elements are arranged by increasing atomic number, there is a periodic repetition of their chemical and physica ...
... • The elements were first organized by increasing atomic mass, which led to inconsistencies. Later, they were organized by increasing atomic number. • The periodic law states that when the elements are arranged by increasing atomic number, there is a periodic repetition of their chemical and physica ...
Document
... the nucleus and repelled by one another. This results in shielding, where an electron is partially shielded from the positive charge of the nucleus by the other electrons. Although all electrons shield one another to some extent, the most effective are the core electrons. As a result, the value o ...
... the nucleus and repelled by one another. This results in shielding, where an electron is partially shielded from the positive charge of the nucleus by the other electrons. Although all electrons shield one another to some extent, the most effective are the core electrons. As a result, the value o ...
Unit 1 Answer Key
... 14. When an organism dies, the amount of C-14 is no longer replenished, so the net ratio of C-14 decreases compared to C-12. Because we know how quickly C-14 decays (is removed from an organism) we can calculate the age of a fossil based on how much C-14 is left in it. ...
... 14. When an organism dies, the amount of C-14 is no longer replenished, so the net ratio of C-14 decreases compared to C-12. Because we know how quickly C-14 decays (is removed from an organism) we can calculate the age of a fossil based on how much C-14 is left in it. ...
Atoms, Nuclear Decay, Electronic Structure, and Atomic Chemical
... The quantum number m l is called the magnetic quantum number. It describes the orientation of the orbital about an x, y, z coordinate system. Each possible orientation can hold up to 2 electrons maximum. For each orbital, there are 2l + 1 different orientations. The quantum number ml is all integer ...
... The quantum number m l is called the magnetic quantum number. It describes the orientation of the orbital about an x, y, z coordinate system. Each possible orientation can hold up to 2 electrons maximum. For each orbital, there are 2l + 1 different orientations. The quantum number ml is all integer ...
Chapter 3
... Elements in the last family, the noble gases, have either two or eight valence electrons. Their most important properties are their extreme stability and lack of reactivity. A full energy level is responsible for this unique stability. The Octet Rule Noble gases are non-reactive because they all hav ...
... Elements in the last family, the noble gases, have either two or eight valence electrons. Their most important properties are their extreme stability and lack of reactivity. A full energy level is responsible for this unique stability. The Octet Rule Noble gases are non-reactive because they all hav ...
Section 2 Electron Configuration and the Periodic Table Chapter 5
... • The number of the highest occupied energy level is 5, so the element is in the fifth period. • There are five electrons in the d sublevel, which means that it is incompletely filled. The d sublevel can hold 10 electrons. Therefore, the element is in the d block. • For d-block elements, the number ...
... • The number of the highest occupied energy level is 5, so the element is in the fifth period. • There are five electrons in the d sublevel, which means that it is incompletely filled. The d sublevel can hold 10 electrons. Therefore, the element is in the d block. • For d-block elements, the number ...
Chapter 3. Elements, Atoms, Ions, and the Periodic Table
... Elements in the last family, the noble gases, have either two or eight valence electrons. Their most important properties are their extreme stability and lack of reactivity. A full energy level is responsible for this unique stability. The Octet Rule Noble gases are non-reactive because they all hav ...
... Elements in the last family, the noble gases, have either two or eight valence electrons. Their most important properties are their extreme stability and lack of reactivity. A full energy level is responsible for this unique stability. The Octet Rule Noble gases are non-reactive because they all hav ...
Chapter3
... Elements in the last family, the noble gases, have either two or eight valence electrons. Their most important properties are their extreme stability and lack of reactivity. A full energy level is responsible for this unique stability. The Octet Rule Noble gases are non-reactive because they all hav ...
... Elements in the last family, the noble gases, have either two or eight valence electrons. Their most important properties are their extreme stability and lack of reactivity. A full energy level is responsible for this unique stability. The Octet Rule Noble gases are non-reactive because they all hav ...
6.3 Periodic Trends
... group. Predicting If a halogen and an alkali metal are in the same period, which one will have the larger radius? Section 6.3 Periodic Trends 171 ...
... group. Predicting If a halogen and an alkali metal are in the same period, which one will have the larger radius? Section 6.3 Periodic Trends 171 ...
The Periodic Table Test Review (3a-3b)
... 16. Identify the representative elements from the list given below. Na, Ca, Sc, Co, Ni, Si, N, Se, Cl, Ge 17. Why is argon placed before potassium in the modern periodic table? 18. Why do elements in the same group have similar properties? 19. Why is the size of a sodium ion (Na+) less than that of ...
... 16. Identify the representative elements from the list given below. Na, Ca, Sc, Co, Ni, Si, N, Se, Cl, Ge 17. Why is argon placed before potassium in the modern periodic table? 18. Why do elements in the same group have similar properties? 19. Why is the size of a sodium ion (Na+) less than that of ...
Jan 26, 2015 - cloudfront.net
... Structure of Matter Each of the more than 100 elements of matter has distinct properties and a distinct atomic structure. All forms of matter are composed of one or more of the elements. As a basis for understanding this concept: Students know the structure of the atom and know it is composed of pro ...
... Structure of Matter Each of the more than 100 elements of matter has distinct properties and a distinct atomic structure. All forms of matter are composed of one or more of the elements. As a basis for understanding this concept: Students know the structure of the atom and know it is composed of pro ...
0321813545_08_final
... For cations, electrons are removed from the highest sublevel of the highest principal energy level. Identify and distinguish between paramagnetic and diamagnetic atoms/ions. Know the relationship between the radius of a neutral atom and its ions: cations are smaller while anions are larger than ...
... For cations, electrons are removed from the highest sublevel of the highest principal energy level. Identify and distinguish between paramagnetic and diamagnetic atoms/ions. Know the relationship between the radius of a neutral atom and its ions: cations are smaller while anions are larger than ...
Periodicity - msmcgartland
... Steps For Drawing Electron Dot Diagrams • Write the atomic symbol for the atom. This will represent the nucleus and the inner energy levels. • Use a dot to represent an outer shell electron. • One dot is placed in each of the four sides before any pairing occurs. • Beginning with the fifth dot, pai ...
... Steps For Drawing Electron Dot Diagrams • Write the atomic symbol for the atom. This will represent the nucleus and the inner energy levels. • Use a dot to represent an outer shell electron. • One dot is placed in each of the four sides before any pairing occurs. • Beginning with the fifth dot, pai ...
Rem001 - The Vital Chemist
... b. Metals have high boiling points and melting points. These increase across a period c. They have relatively high densities which increase down a group and from left to right. The properties above are due to the strong electrostatic force of attraction between electron could and metallic ions (meta ...
... b. Metals have high boiling points and melting points. These increase across a period c. They have relatively high densities which increase down a group and from left to right. The properties above are due to the strong electrostatic force of attraction between electron could and metallic ions (meta ...
NC SCS Chemistry
... Identify periods as horizontal rows on the periodic table Know that main group elements in the same family have similar properties, the same number of valence electrons, and the same oxidation number Understand that reactivity increases down in a group of metals and decrease down in a group of nonme ...
... Identify periods as horizontal rows on the periodic table Know that main group elements in the same family have similar properties, the same number of valence electrons, and the same oxidation number Understand that reactivity increases down in a group of metals and decrease down in a group of nonme ...
Notes Trends in the Periodic Table
... Why does atomic radius increase from top to bottom in a chemical family? Nuclear charge increases from top to bottom in a chemical family. Nuclear charge decreases from top to bottom in a chemical family. The number of energy levels increases from top to bottom in a chemical family. The number of en ...
... Why does atomic radius increase from top to bottom in a chemical family? Nuclear charge increases from top to bottom in a chemical family. Nuclear charge decreases from top to bottom in a chemical family. The number of energy levels increases from top to bottom in a chemical family. The number of en ...
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.