Background Information: The periodic table is arranged in order of
... contain the same number of electrons but an increasing number of protons so the ionic radius decreases in size. The anions (P3-, S2- and Cl-) contain more electrons than protons and therefore are larger than the parent atom. Across a period, the ionic size decreases because the number of electrons r ...
... contain the same number of electrons but an increasing number of protons so the ionic radius decreases in size. The anions (P3-, S2- and Cl-) contain more electrons than protons and therefore are larger than the parent atom. Across a period, the ionic size decreases because the number of electrons r ...
periodic-trends_atomic-and-ionic-radii
... contain the same number of electrons but an increasing number of protons so the ionic radius decreases in size. The anions (P3-, S2- and Cl-) contain more electrons than protons and therefore are larger than the parent atom. Across a period, the ionic size decreases because the number of electrons r ...
... contain the same number of electrons but an increasing number of protons so the ionic radius decreases in size. The anions (P3-, S2- and Cl-) contain more electrons than protons and therefore are larger than the parent atom. Across a period, the ionic size decreases because the number of electrons r ...
Unit 4 Powerpoint Notes
... and are soft enough to cut with a knife. • They are extremely reactive and are not found in nature as free elements. • They must be stored under oil or kerosene. ...
... and are soft enough to cut with a knife. • They are extremely reactive and are not found in nature as free elements. • They must be stored under oil or kerosene. ...
Ch. 7 Sections 7.10 and 7.12 Note Organizer
... Why is I1 _________________ than I2? The first electron is removed from a ______________ atom and the second is removed from a 1+ ____________. The ________________ in ______________ charge binds the electrons more firmly and it takes more energy to remove an electron. Why is I4 so high? The fourth ...
... Why is I1 _________________ than I2? The first electron is removed from a ______________ atom and the second is removed from a 1+ ____________. The ________________ in ______________ charge binds the electrons more firmly and it takes more energy to remove an electron. Why is I4 so high? The fourth ...
Chapter 7 Periodic Properties of the Elements
... additional e- is paired with 1 of the 3 p e- The proximity of two e- in the same orbital leads to high electrostatic repulsion, which makes it easier to ionize an atom of the Group 6A element, even though the nuclear charge has increased by one unit. ...
... additional e- is paired with 1 of the 3 p e- The proximity of two e- in the same orbital leads to high electrostatic repulsion, which makes it easier to ionize an atom of the Group 6A element, even though the nuclear charge has increased by one unit. ...
Learning Guide 3
... 4. As you go down a group the elements may change from nonmetal metalloid metal. 5. The metallic characteristics increase as you go down a group. 6. As you go left to right metallic characteristics ...
... 4. As you go down a group the elements may change from nonmetal metalloid metal. 5. The metallic characteristics increase as you go down a group. 6. As you go left to right metallic characteristics ...
How can atomic theory explain patterns in the periodic table?
... properties of that element. For example, an atom of carbon is represented in Figure 2.15. Each atom has a tiny, dense nucleus containing neutrons and protons. (A hydrogen nucleus has a single proton only.) The nucleus is surrounded by electrons, which exist in specific electron energy shells. Most o ...
... properties of that element. For example, an atom of carbon is represented in Figure 2.15. Each atom has a tiny, dense nucleus containing neutrons and protons. (A hydrogen nucleus has a single proton only.) The nucleus is surrounded by electrons, which exist in specific electron energy shells. Most o ...
The Periodic Table
... The third shell is filled across the period from left to right. What is special about the outer shell of argon? 28 of 39 ...
... The third shell is filled across the period from left to right. What is special about the outer shell of argon? 28 of 39 ...
Trends_in_the_Periodic_Table_1_
... Group - electronegativity decreases as you go down a group. Why? Elements near the top of the period table have few electrons to begin with; every electron is a big deal. They have a stronger desire to acquire more electrons. Elements near the bottom of the chart have so many electrons that loosing ...
... Group - electronegativity decreases as you go down a group. Why? Elements near the top of the period table have few electrons to begin with; every electron is a big deal. They have a stronger desire to acquire more electrons. Elements near the bottom of the chart have so many electrons that loosing ...
The Periodic Table
... a. Zeff = # protons - # core (non-valence) electrons 3. Electron shielding- the inner electrons ______________ the outer electrons from some of the nucleus’ ___________________ force. a. Going down a group adds another ___________________ energy level adds more shielding. B. Periodic trends are __ ...
... a. Zeff = # protons - # core (non-valence) electrons 3. Electron shielding- the inner electrons ______________ the outer electrons from some of the nucleus’ ___________________ force. a. Going down a group adds another ___________________ energy level adds more shielding. B. Periodic trends are __ ...
Trends of the Periodic Table
... Why? Elements on the right of the chart want electrons (not giving them up) because they are close to achieving the octet. That means it will require more energy to remove the outer most electron. Elements on the left of the chart would prefer to give up their electrons so it is easy to remove them, ...
... Why? Elements on the right of the chart want electrons (not giving them up) because they are close to achieving the octet. That means it will require more energy to remove the outer most electron. Elements on the left of the chart would prefer to give up their electrons so it is easy to remove them, ...
Document
... For Groups 1, 2, and 13-18 on the Periodic Table, elements within the same group have the same number of valence electrons (helium is an exception) and therefore similar chemical properties. ...
... For Groups 1, 2, and 13-18 on the Periodic Table, elements within the same group have the same number of valence electrons (helium is an exception) and therefore similar chemical properties. ...
Appendices: Cluster 2 Atoms and Elements
... • Lavoisier defined the term “element” as a pure substance that cannot be chemically broken down into simpler substances. • He discovered and identified 23 elements. He based his investigations on careful measurement and observations. • He recognized mixtures exist and identified air as a mixture of ...
... • Lavoisier defined the term “element” as a pure substance that cannot be chemically broken down into simpler substances. • He discovered and identified 23 elements. He based his investigations on careful measurement and observations. • He recognized mixtures exist and identified air as a mixture of ...
Ch. 17 PPT
... lined up according to their chemical properties. • He looked at the properties and atomic masses of the elements surrounding these ...
... lined up according to their chemical properties. • He looked at the properties and atomic masses of the elements surrounding these ...
periodic table - Cloudfront.net
... lined up according to their chemical properties. • He looked at the properties and atomic masses of the elements surrounding these ...
... lined up according to their chemical properties. • He looked at the properties and atomic masses of the elements surrounding these ...
The Periodic Table and Periodic Trends
... • Dull, brittle substances that are poor conductors of heat and electricity. • Tend to gain electrons in reactions with metals to acquire noble gas configuration. ...
... • Dull, brittle substances that are poor conductors of heat and electricity. • Tend to gain electrons in reactions with metals to acquire noble gas configuration. ...
Periodicity Chemistry Worksheet
... 5. Along with the increased distance of the outer electrons from the nucleus, the _Shielding Effect__ of the inner electrons causes ionization energy to decrease going down a column of the periodic table. 6. A low ionization energy is characteristic of a(n) _Metals_______________________. 7. Ionizat ...
... 5. Along with the increased distance of the outer electrons from the nucleus, the _Shielding Effect__ of the inner electrons causes ionization energy to decrease going down a column of the periodic table. 6. A low ionization energy is characteristic of a(n) _Metals_______________________. 7. Ionizat ...
basic atomic structure power point File
... • Originally constructed to represent the patterns observed in the chemical properties of the elements. • Mendeleev is given the most credit for the current version of the periodic table. • Elements are ordered by atomic number (protons). • Elements w/i a group have similar properties. ...
... • Originally constructed to represent the patterns observed in the chemical properties of the elements. • Mendeleev is given the most credit for the current version of the periodic table. • Elements are ordered by atomic number (protons). • Elements w/i a group have similar properties. ...
Introduction to Atoms
... 6. A material that is ________________________ can be hammered into sheets and other shapes. 7. A powerful machine called a(n) ________________________ moves nuclear particles fast enough to make larger nuclei when the particles collide. 8. The ability to transmit heat or electricity to other object ...
... 6. A material that is ________________________ can be hammered into sheets and other shapes. 7. A powerful machine called a(n) ________________________ moves nuclear particles fast enough to make larger nuclei when the particles collide. 8. The ability to transmit heat or electricity to other object ...
Study Guide - Rochester Century High School
... • Alkaline earth metal • Group • Halogen • Inner transition metal • Lanthanide series • Metal • Metalloid • Noble gas • Nonmetal • Period • Periodic law • Representative element • Transition element • Transition metal ...
... • Alkaline earth metal • Group • Halogen • Inner transition metal • Lanthanide series • Metal • Metalloid • Noble gas • Nonmetal • Period • Periodic law • Representative element • Transition element • Transition metal ...
Ch. 7 Sections 7.10 and 7.12 Powerpoint
... right across a period. A valence shell that holds its electrons tightly will also tend to bind an additional electron tightly. •Electron affinity becomes less negative down a group. A valence shell that loses electrons easily (low IE) will have little attraction for additional electrons (small EA). ...
... right across a period. A valence shell that holds its electrons tightly will also tend to bind an additional electron tightly. •Electron affinity becomes less negative down a group. A valence shell that loses electrons easily (low IE) will have little attraction for additional electrons (small EA). ...
The Periodic Table: Electron Shells Affect Trends
... 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(eight the outer shell) ...
... 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(eight the outer shell) ...
PreAP Chemistry Chapter 5 Notes
... these elements were found quickly, while others were not found until after his death due to their highly radioactive (unstable) nature. ...
... these elements were found quickly, while others were not found until after his death due to their highly radioactive (unstable) nature. ...
D. - Telluride Middle/High School
... The s-, p-, d-, and f-Block Elements • The shape of the periodic table becomes clear if it is divided into blocks representing the atom’s energy sublevel being filled with valence electrons. ...
... The s-, p-, d-, and f-Block Elements • The shape of the periodic table becomes clear if it is divided into blocks representing the atom’s energy sublevel being filled with valence electrons. ...
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.