Periodic Table
... ii) Compare the periodic trends of atomic radii, ionization energy, and electronegativity, and state the reasons for these variations. iii) Define valence electrons, and state how many are present in atoms of each main-group element. ...
... ii) Compare the periodic trends of atomic radii, ionization energy, and electronegativity, and state the reasons for these variations. iii) Define valence electrons, and state how many are present in atoms of each main-group element. ...
Section 4.4*The Periodic Table
... • All nonmetals exist as gases nonreactive elements- most stable Called inert gases All have 8 valence electrons except Helium which only has 2 and does not form ions ...
... • All nonmetals exist as gases nonreactive elements- most stable Called inert gases All have 8 valence electrons except Helium which only has 2 and does not form ions ...
Skills you should have mastered
... If more than one orbital in a subshell is available, add electrons with parallel spin to different orbitals of that subshell rather than pairing two electrons in one of them. ...
... If more than one orbital in a subshell is available, add electrons with parallel spin to different orbitals of that subshell rather than pairing two electrons in one of them. ...
Section 4.3 Guided Notes
... _____________in the energy levels between the _______________ and the __________________ electrons. This is called electron shielding. d. Electron Shielding: the ___________________ of the attractive force between a positively charged _______________ and its outermost ________________ due to the can ...
... _____________in the energy levels between the _______________ and the __________________ electrons. This is called electron shielding. d. Electron Shielding: the ___________________ of the attractive force between a positively charged _______________ and its outermost ________________ due to the can ...
Chem 0910-040
... The alkali and alkaline-earth metals are the least electronegative elements. In compounds, their atoms have a low attraction for electrons. Nitrogen, oxygen, and the halogens are the most electronegative elements. Their atoms attract electrons strongly in compounds. ...
... The alkali and alkaline-earth metals are the least electronegative elements. In compounds, their atoms have a low attraction for electrons. Nitrogen, oxygen, and the halogens are the most electronegative elements. Their atoms attract electrons strongly in compounds. ...
Unit 3 Notes
... Similarities occur because elements in the same group have the same number of valence electrons Valence electrons determine many of the properties of an element ...
... Similarities occur because elements in the same group have the same number of valence electrons Valence electrons determine many of the properties of an element ...
Document
... _____________in the energy levels between the _______________ and the __________________ electrons. This is called electron shielding. d. Electron Shielding: the ___________________ of the attractive force between a positively charged _______________ and its outermost ________________ due to the can ...
... _____________in the energy levels between the _______________ and the __________________ electrons. This is called electron shielding. d. Electron Shielding: the ___________________ of the attractive force between a positively charged _______________ and its outermost ________________ due to the can ...
Elements and the Periodic Table
... Organizing the Elements Metals Nonmetals and Metalloids Elements From Stardust ...
... Organizing the Elements Metals Nonmetals and Metalloids Elements From Stardust ...
2+ - West Ada
... - All are metals that react readily with nonmetals to give ions with a 2 charge. ...
... - All are metals that react readily with nonmetals to give ions with a 2 charge. ...
Lesson Objectives Vocabulary Introduction
... attraction is weakened by shielding, the valence shell cannot be pulled in as close. The more shielding that occurs, the further the valence shell can spread out. For example, if you are looking at the element sodium, it has the electron configuration: ...
... attraction is weakened by shielding, the valence shell cannot be pulled in as close. The more shielding that occurs, the further the valence shell can spread out. For example, if you are looking at the element sodium, it has the electron configuration: ...
Metals and Nonmetals Metals and Nonmetals
... – Includes the noble (inert) gases as a special case ...
... – Includes the noble (inert) gases as a special case ...
What happens down a group?
... • Found in group 18 (the last column of the periodic table.) • Do not react easily with other elements, as they have a full outer shell. ...
... • Found in group 18 (the last column of the periodic table.) • Do not react easily with other elements, as they have a full outer shell. ...
Periodic Trends
... region occupied by the 1s electron. 2s electron experiences a higher positive charge than expected. ...
... region occupied by the 1s electron. 2s electron experiences a higher positive charge than expected. ...
Periodic Trends - killingly.k12.ct.us
... elements on the right side of the periodic table are more energy-efficient in gaining electrons to create a complete valence shell of 8 electrons. This effectively describes the nature of electronegativity: the more inclined an atom is to gain electrons, the more likely that atom will pull electrons ...
... elements on the right side of the periodic table are more energy-efficient in gaining electrons to create a complete valence shell of 8 electrons. This effectively describes the nature of electronegativity: the more inclined an atom is to gain electrons, the more likely that atom will pull electrons ...
The electronic structure of atoms of the elements
... postulated that the behaviour of electrons in atoms could be described by mathematical equations similar to those used to describe the motion of standing waves in a string. From this model the electrons can be visualised as electron clouds of various shapes with the nucleus of the atom at their cent ...
... postulated that the behaviour of electrons in atoms could be described by mathematical equations similar to those used to describe the motion of standing waves in a string. From this model the electrons can be visualised as electron clouds of various shapes with the nucleus of the atom at their cent ...
Physical Science Comprehensive Fall 2010 SAMPLE QUESTIONS
... 12. According to the periodic table, the group known as the halogens include the element: A. sodium. B. calcium. C. chlorine. D. phosphorus. 13. Using the periodic table, transition elements belong to groups: A. 1-8 B. 3-12 C. 10-15 D. 13-18 14. Using the periodic table, all of the following element ...
... 12. According to the periodic table, the group known as the halogens include the element: A. sodium. B. calcium. C. chlorine. D. phosphorus. 13. Using the periodic table, transition elements belong to groups: A. 1-8 B. 3-12 C. 10-15 D. 13-18 14. Using the periodic table, all of the following element ...
Periodic Relationships
... Most important tool in chemistry Key to understanding chemical and physical properties Each group has same electron configuration for outer shell. ...
... Most important tool in chemistry Key to understanding chemical and physical properties Each group has same electron configuration for outer shell. ...
Catalyst
... Catalyst 1. Open up the Bohr’s Model educanon video for today’s class. Complete the questions associated with the video. 2. Put your laptop at 45 degrees and place your eyes on me so I know when you’re finished. ...
... Catalyst 1. Open up the Bohr’s Model educanon video for today’s class. Complete the questions associated with the video. 2. Put your laptop at 45 degrees and place your eyes on me so I know when you’re finished. ...
Chemical Periodicity
... 2. Who is Dmitri Mendeleev, and what was his contribution to chemistry? 3. How is the modern periodic table different from the first periodic table? 4. What is the modern periodic law? 5. Organization of the periodic table. Indicate where the following are located on the periodic table. h. Transitio ...
... 2. Who is Dmitri Mendeleev, and what was his contribution to chemistry? 3. How is the modern periodic table different from the first periodic table? 4. What is the modern periodic law? 5. Organization of the periodic table. Indicate where the following are located on the periodic table. h. Transitio ...
The Periodic Table
... • All matter is made up of atoms, which are far too small to see directly through a microscope. The atoms of any element are alike but are different from atoms of other elements. Atoms may stick together in well-defined molecules or may be packed together in large arrays. Different arrangements of a ...
... • All matter is made up of atoms, which are far too small to see directly through a microscope. The atoms of any element are alike but are different from atoms of other elements. Atoms may stick together in well-defined molecules or may be packed together in large arrays. Different arrangements of a ...
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.