Ch 6 Notes
... increased nuclear charge pulls the outermost electrons ___________________ to the nucleus, making the atom _____________________. 24. As you move down a group, atomic radii __________________________. This is due to the addition of a larger energy ___________________ each time. Electrons in higher l ...
... increased nuclear charge pulls the outermost electrons ___________________ to the nucleus, making the atom _____________________. 24. As you move down a group, atomic radii __________________________. This is due to the addition of a larger energy ___________________ each time. Electrons in higher l ...
Packet 4 - 16-17 Periodic Table
... Two or more forms of the same element that differ in their molecules. Allotropes have different properties. Oxygen has 2 allotropes: O2 is the oxygen we breathe, and O3 makes up the ozone layer. Carbon has many different allotropes which differ in arrangement of atoms • Diamond: every carbon bonded ...
... Two or more forms of the same element that differ in their molecules. Allotropes have different properties. Oxygen has 2 allotropes: O2 is the oxygen we breathe, and O3 makes up the ozone layer. Carbon has many different allotropes which differ in arrangement of atoms • Diamond: every carbon bonded ...
The Periodic Table
... Copper, Cu, is a relatively soft metal, and a very good electrical conductor. ...
... Copper, Cu, is a relatively soft metal, and a very good electrical conductor. ...
Periodic Table Development
... electrons start to be located in f orbitals f orbitals can hold 14 electrons start filling 4f orbitals on 6 period with La (atomic # 57) f – block elements called inner transition metals Periodic Table shape is due to the way electrons fill s,p,d, f orbitals of different energy levels ...
... electrons start to be located in f orbitals f orbitals can hold 14 electrons start filling 4f orbitals on 6 period with La (atomic # 57) f – block elements called inner transition metals Periodic Table shape is due to the way electrons fill s,p,d, f orbitals of different energy levels ...
Physical Science 100 Chapter 18, The Periodic Table
... Metals and non-metals are separated by a red “staircase” Elements near this staircase are called semi-metals (or semi-conductors) The noble or inert gases are on the far right. ...
... Metals and non-metals are separated by a red “staircase” Elements near this staircase are called semi-metals (or semi-conductors) The noble or inert gases are on the far right. ...
Atoms in the Periodic Table
... The family of noble gases includes helium, neon, argon, krypton, xenon, and radon. All the noble gases are found in small amounts in the earth's atmosphere. ...
... The family of noble gases includes helium, neon, argon, krypton, xenon, and radon. All the noble gases are found in small amounts in the earth's atmosphere. ...
Unit #4 Periodic Table Families Notes
... occurrence and chemical properties of elements which had not yet been discovered. ...
... occurrence and chemical properties of elements which had not yet been discovered. ...
The Modern Periodic Table
... Modern Periodic law: “The physical & chemical properties of elements are the periodic functions of the electron configuration of their atoms.” The modern Periodic table consists of 7 Horizontal rows called periods and 18 vertical columns called groups or families. • The first period is the smallest ...
... Modern Periodic law: “The physical & chemical properties of elements are the periodic functions of the electron configuration of their atoms.” The modern Periodic table consists of 7 Horizontal rows called periods and 18 vertical columns called groups or families. • The first period is the smallest ...
View PDF
... 7. Define electronegativity, ionization energy, atomic radius, and electron affinity: Electronegativity – the ability of an atom to attract electrons towards itself increases across a period, decreases down a group Ionization energy – the energy required to remove an electron from an atom increases ...
... 7. Define electronegativity, ionization energy, atomic radius, and electron affinity: Electronegativity – the ability of an atom to attract electrons towards itself increases across a period, decreases down a group Ionization energy – the energy required to remove an electron from an atom increases ...
Ch 6 Notes
... However, once you remove the first electron, much more energy is required to remove the second, and third, and fourth, etc. ...
... However, once you remove the first electron, much more energy is required to remove the second, and third, and fourth, etc. ...
Periodic Law Power Point
... the electrons more strongly than the other. The uneven concentration of charge has a significant effect on the chemical properties of a compound and therefore it is useful to have a measure of how strongly one atom attracts the electrons of another atom within a ...
... the electrons more strongly than the other. The uneven concentration of charge has a significant effect on the chemical properties of a compound and therefore it is useful to have a measure of how strongly one atom attracts the electrons of another atom within a ...
The History of the Modern Periodic Table
... Valence Electrons • electrons available to be lost, gained, or shared in the formation of chemical compounds • usually in the outermost s and p orbitals for main group elements (Families 1 & 2, and Families 13-18) ...
... Valence Electrons • electrons available to be lost, gained, or shared in the formation of chemical compounds • usually in the outermost s and p orbitals for main group elements (Families 1 & 2, and Families 13-18) ...
Trends PPP#1
... the electrons more strongly than the other. The uneven concentration of charge has a significant effect on the chemical properties of a compound and therefore it is useful to have a measure of how strongly one atom attracts the electrons of another atom within a ...
... the electrons more strongly than the other. The uneven concentration of charge has a significant effect on the chemical properties of a compound and therefore it is useful to have a measure of how strongly one atom attracts the electrons of another atom within a ...
Slide 1
... There is an s-block, p-block, d-block, and f-block. S-block is group 1 and 2. Group 1 electron configurations end with ns1, group 2 end with ns2. P-block is group 13 through 18. Electron configurations proceed as np1, np2, np3, np4, np5, and np6. The n in each electron configuration indicates the ma ...
... There is an s-block, p-block, d-block, and f-block. S-block is group 1 and 2. Group 1 electron configurations end with ns1, group 2 end with ns2. P-block is group 13 through 18. Electron configurations proceed as np1, np2, np3, np4, np5, and np6. The n in each electron configuration indicates the ma ...
Periodic Trends Notes
... •Elements within the same period have the same number of energy levels and therefore the same shielding effect. •As you move toward the right, the nuclear charge increases. •With more nuclear charge, and no increase in shielding, the outermost electrons are drawn closer to the nucleus, and hence the ...
... •Elements within the same period have the same number of energy levels and therefore the same shielding effect. •As you move toward the right, the nuclear charge increases. •With more nuclear charge, and no increase in shielding, the outermost electrons are drawn closer to the nucleus, and hence the ...
Chapter 6 Test - The Periodic Table
... ____ 12. Each period in the periodic table corresponds to ____. a. an orbital c. an energy level b. a suborbital d. an energy sublevel ____ 13. The modern periodic table is arranged in order of increasing atomic ____. a. radius c. charge b. number d. mass ____ 14. Who arranged the elements according ...
... ____ 12. Each period in the periodic table corresponds to ____. a. an orbital c. an energy level b. a suborbital d. an energy sublevel ____ 13. The modern periodic table is arranged in order of increasing atomic ____. a. radius c. charge b. number d. mass ____ 14. Who arranged the elements according ...
History of the Periodic Table
... block structure of the periodic table. For convenience hydrogen is usually placed on top of Group 1 although it is not considered an alkali metal. ...
... block structure of the periodic table. For convenience hydrogen is usually placed on top of Group 1 although it is not considered an alkali metal. ...
Chapter 3 Section 2 Notes
... extremely active solid. The last element in a period, is always an inactive gas. ...
... extremely active solid. The last element in a period, is always an inactive gas. ...
The Periodic Table
... The Periodic Table Aluminum is a representative element. Copper is a transition metal. Na is an _______________________ Mg is an _______________________ F is a ________________________ Ne is a ______________________ Ag is a ______________________ ...
... The Periodic Table Aluminum is a representative element. Copper is a transition metal. Na is an _______________________ Mg is an _______________________ F is a ________________________ Ne is a ______________________ Ag is a ______________________ ...
The Periodic Table
... Said properties of unknown elements could be predicted by the properties of elements around the missing element ...
... Said properties of unknown elements could be predicted by the properties of elements around the missing element ...
Ch.6 Periodic Trends - MrsSavallisChemistry
... 1. What property did Mendeleev use to organize his periodic table? 2. How are elements arranged on the modern periodic table? 3. Name the three broad classes of elements. 4. Identify each property below as more characteristic of a mental or a nonmetal. a. a gas b. brittle c. malleable d. poor conduc ...
... 1. What property did Mendeleev use to organize his periodic table? 2. How are elements arranged on the modern periodic table? 3. Name the three broad classes of elements. 4. Identify each property below as more characteristic of a mental or a nonmetal. a. a gas b. brittle c. malleable d. poor conduc ...
A scientist named Henry Mosley developed the modern period table
... Use your science notes and chapter 6 of the science textbook while completing the following section. 1. Compare the way Mendeleev and Moseley organized the periodic table. Hint… we use Moseley’s periodic table today. ...
... Use your science notes and chapter 6 of the science textbook while completing the following section. 1. Compare the way Mendeleev and Moseley organized the periodic table. Hint… we use Moseley’s periodic table today. ...
questions on periodic classification of elements
... 11. The elements Li, Be, B , C ,N, O ,F and Ne are present in the second period . How many valence electrons do these elements have? Classify them as metals and non metals. 12. An atom ‘X’ has electronic configuration 2,8,7. a)What is the atomic number of this element? b) State whether ‘X’ is a meta ...
... 11. The elements Li, Be, B , C ,N, O ,F and Ne are present in the second period . How many valence electrons do these elements have? Classify them as metals and non metals. 12. An atom ‘X’ has electronic configuration 2,8,7. a)What is the atomic number of this element? b) State whether ‘X’ is a meta ...
File - dr. stephen alfred
... 11. Each column of the Periodic Table is called a ________. The Elements in a group have __________________________________. 12. Elements on the left of the Periodic Table are _________________________, ____________________ in the middle, ______________ on the right. ...
... 11. Each column of the Periodic Table is called a ________. The Elements in a group have __________________________________. 12. Elements on the left of the Periodic Table are _________________________, ____________________ in the middle, ______________ on the right. ...
Group 3 element
Group 3 is a group of elements in the periodic table. This group, like other d-block groups, should contain four elements, but it is not agreed what elements belong in the group. Scandium (Sc) and yttrium (Y) are always included, but the other two spaces are usually occupied by lanthanum (La) and actinium (Ac), or by lutetium (Lu) and lawrencium (Lr); less frequently, it is considered the group should be expanded to 32 elements (with all the lanthanides and actinides included) or contracted to contain only scandium and yttrium. The group itself has not acquired a trivial name; however, scandium, yttrium and the lanthanides are sometimes called rare earth metals.Three group 3 elements occur naturally, scandium, yttrium, and either lanthanum or lutetium. Lanthanum continues the trend started by two lighter members in general chemical behavior, while lutetium behaves more similarly to yttrium. This is in accordance with the trend for period 6 transition metals to behave more similarly to their upper periodic table neighbors. This trend is seen from hafnium, which is almost identical chemically to zirconium, to mercury, which is quite distant chemically from cadmium, but still shares with it almost equal atomic size and other similar properties. They all are silvery-white metals under standard conditions. The fourth element, either actinium or lawrencium, has only radioactive isotopes. Actinium, which occurs only in trace amounts, continues the trend in chemical behavior for metals that form tripositive ions with a noble gas configuration; synthetic lawrencium is calculated and partially shown to be more similar to lutetium and yttrium. So far, no experiments have been conducted to synthesize any element that could be the next group 3 element. Unbiunium (Ubu), which could be considered a group 3 element if preceded by lanthanum and actinium, might be synthesized in the near future, it being only three spaces away from the current heaviest element known, ununoctium.