columns
... the nuclear charge, so the attraction between the nucleus and electrons is weaker and the atom expands in size. In contrast, atoms get smaller as you go across the periods because the nuclear charge effect outweighs the shielding effect, so the attraction between the nucleus and the electron is grea ...
... the nuclear charge, so the attraction between the nucleus and electrons is weaker and the atom expands in size. In contrast, atoms get smaller as you go across the periods because the nuclear charge effect outweighs the shielding effect, so the attraction between the nucleus and the electron is grea ...
CHEM121 Lecture Ch2-3
... – primary substances from which all other things are built. – Cannot be broken down into simpler substances ...
... – primary substances from which all other things are built. – Cannot be broken down into simpler substances ...
Study Guide
... particles that carry a positive charge. Neutrons are particles that carry no electric charge. The nucleus is the center of the atom that is made up of both protons and neutrons. Electrons are particles that carry a negative charge and surround the nucleus in what is know as the electron cloud on ene ...
... particles that carry a positive charge. Neutrons are particles that carry no electric charge. The nucleus is the center of the atom that is made up of both protons and neutrons. Electrons are particles that carry a negative charge and surround the nucleus in what is know as the electron cloud on ene ...
Physical Science 100 Chapter 18, The Periodic Table
... Mendeleev created a table with elements arranged by atomic weights. He noted behaviors of chemical properties that appeared to be periodic in weights. Chemical Similarity in Families • chemical behavior is dictated by the “valence” electrons • the number of valence electrons is the same for elements ...
... Mendeleev created a table with elements arranged by atomic weights. He noted behaviors of chemical properties that appeared to be periodic in weights. Chemical Similarity in Families • chemical behavior is dictated by the “valence” electrons • the number of valence electrons is the same for elements ...
THE PERIODIC TABLE Introduction • Dmitri Mendeleev is the father
... modern periodic table appeared. • The modern periodic table contains physical and chemical properties of elements. It is arranged according to increasing atomic numbers. • Horizontal rows are called periods. There are 7 periods beginning with a metal and ending with a noble gas. • Vertical columns a ...
... modern periodic table appeared. • The modern periodic table contains physical and chemical properties of elements. It is arranged according to increasing atomic numbers. • Horizontal rows are called periods. There are 7 periods beginning with a metal and ending with a noble gas. • Vertical columns a ...
Questions on The Periodic Table
... 6. What were the problems that arose when more elements were discovered are more accurate atomic weights determined? Give examples. 7.What are the three particles making up the atom, their mass, charge and location? 8. What is the mass number of an atom? 9. What is the atomic number of an atom and w ...
... 6. What were the problems that arose when more elements were discovered are more accurate atomic weights determined? Give examples. 7.What are the three particles making up the atom, their mass, charge and location? 8. What is the mass number of an atom? 9. What is the atomic number of an atom and w ...
graphing atomic properties
... ----------------Circle the correct answer(s) in the brackets below.---------------8. Going across a period from left to right: The [ p+, N0, e- ] in the nucleus increase, thus pulling the [ p+ , N0, e- ] closer towards the center of the atom and [ increasing, decreasing ] the atomic radii. Because o ...
... ----------------Circle the correct answer(s) in the brackets below.---------------8. Going across a period from left to right: The [ p+, N0, e- ] in the nucleus increase, thus pulling the [ p+ , N0, e- ] closer towards the center of the atom and [ increasing, decreasing ] the atomic radii. Because o ...
Unit 3 `Atoms and the Periodic Table` Study Guide
... known elements. Products – the results of a chemical reaction Proton – a subatomic particle identical with the nucleus of the hydrogen atom; found with neutrons in all atomic nuclei; carries a positive charge. Reactants – the starting materials for a reaction Replacement Reaction – chemical reaction ...
... known elements. Products – the results of a chemical reaction Proton – a subatomic particle identical with the nucleus of the hydrogen atom; found with neutrons in all atomic nuclei; carries a positive charge. Reactants – the starting materials for a reaction Replacement Reaction – chemical reaction ...
Ch.4 Notes Powerpoint Version
... • Recall that groups 1 and 7 are the most reactive metals and nonmetals. • As we move down group 1, the alkali metals become more reactive- this is because of the trend seen in ionization energy! • As we move down group 7, the halogens become less reactive- this is because of the trend seen in elect ...
... • Recall that groups 1 and 7 are the most reactive metals and nonmetals. • As we move down group 1, the alkali metals become more reactive- this is because of the trend seen in ionization energy! • As we move down group 7, the halogens become less reactive- this is because of the trend seen in elect ...
Atomic Structure Test – Study Guide
... 7. Sodium wants to bond with chlorine because it has only ____ valence electron. It wants to _____ that electron to Chlorine. Chlorine wants to take that electron because it has ____ valence electrons and so only needs ____ more electron to have a filled outer level. Chemical Reactions Explain why m ...
... 7. Sodium wants to bond with chlorine because it has only ____ valence electron. It wants to _____ that electron to Chlorine. Chlorine wants to take that electron because it has ____ valence electrons and so only needs ____ more electron to have a filled outer level. Chemical Reactions Explain why m ...
Periodic Table and Trends
... [why is it +1? If you look at Li, Li has 3 protons, so it must have 3 electrons. To get to the nearest noble gas, helium, Li would have to lose 1 electron. ...
... [why is it +1? If you look at Li, Li has 3 protons, so it must have 3 electrons. To get to the nearest noble gas, helium, Li would have to lose 1 electron. ...
Atoms & Elements
... Structure of atom: An atom consists • of a nucleus that contains protons and neutrons. • of electrons in a large empty space around the nucleus. • a proton has a mass of about 1 (1.007) amu. • a neutron has a mass of about 1 (1.008) amu. • an electron has a very small mass, 0.000549 amu. ...
... Structure of atom: An atom consists • of a nucleus that contains protons and neutrons. • of electrons in a large empty space around the nucleus. • a proton has a mass of about 1 (1.007) amu. • a neutron has a mass of about 1 (1.008) amu. • an electron has a very small mass, 0.000549 amu. ...
HS standard 4 2017
... Think about metals. Metals are typically shiny (luster) and are solid. Gases obviously do not fit this description. All the common gases are non-metals which are found in the upper right corner. ...
... Think about metals. Metals are typically shiny (luster) and are solid. Gases obviously do not fit this description. All the common gases are non-metals which are found in the upper right corner. ...
In the periodic table, the elements are placed from left to right in
... particularly that of the valence shell electrons. For instance, all atoms with four valence electrons occupying p orbitals will share some similar characteristics. The type of orbital in which the atom's outermost electrons reside determines the "block" to which that element belongs. The number of v ...
... particularly that of the valence shell electrons. For instance, all atoms with four valence electrons occupying p orbitals will share some similar characteristics. The type of orbital in which the atom's outermost electrons reside determines the "block" to which that element belongs. The number of v ...
Chapter 6 Powerpoint
... 1. Into what four classes can elements be sorted based on their electron configuration? 2. Why do the elements potassium and sodium have similar chemical properties? ...
... 1. Into what four classes can elements be sorted based on their electron configuration? 2. Why do the elements potassium and sodium have similar chemical properties? ...
Chapter 5 The Periodic Law
... has 8 (octet) electrons in the highest energy level except He which has 2 charge of 0 ...
... has 8 (octet) electrons in the highest energy level except He which has 2 charge of 0 ...
Document
... • Mendeleev arranged the Periodic Table by? • Today’s Periodic Table is arranged by? • Know how to read the Periodic Table. • Be able to give the atomic mass, atomic number, symbol for a given element. Given a symbol, be able to give the name of the element. ...
... • Mendeleev arranged the Periodic Table by? • Today’s Periodic Table is arranged by? • Know how to read the Periodic Table. • Be able to give the atomic mass, atomic number, symbol for a given element. Given a symbol, be able to give the name of the element. ...
Unit 4: The Periodic Table and Periodicity Name - Teach-n
... 12. Why is the symbol for sodium printed in black? sodium is a solid at room temperature 13. List the chemical symbols of all of the… ...
... 12. Why is the symbol for sodium printed in black? sodium is a solid at room temperature 13. List the chemical symbols of all of the… ...
Chapter 6 Review Name Period _____ Know the history
... With the addition of an electron the repulsion between the electrons increases increasing the size of the ion. 33. When an atom becomes a cation, what happens to its radius? Why? As an atom loses an electron the repulsion decreases 34. For each of the following pairs, circle the atom or ion having t ...
... With the addition of an electron the repulsion between the electrons increases increasing the size of the ion. 33. When an atom becomes a cation, what happens to its radius? Why? As an atom loses an electron the repulsion decreases 34. For each of the following pairs, circle the atom or ion having t ...
CH 5 Section Review 1-3
... 4. Elements in a group, or column, in the Periodic Table can be expected to have similar (a) atomic masses; (b) atomic numbers; (c) numbers of neutrons; (d) properties. 5. The radioactive elements with atomic numbers from 90 to 103 in the Periodic Table are referred to as the (a) noble gases; (b) la ...
... 4. Elements in a group, or column, in the Periodic Table can be expected to have similar (a) atomic masses; (b) atomic numbers; (c) numbers of neutrons; (d) properties. 5. The radioactive elements with atomic numbers from 90 to 103 in the Periodic Table are referred to as the (a) noble gases; (b) la ...
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.