Periodic Trends Review Sheet
... 9. Is it easier to form a positive ion with an element that has a high ionization energy or an element that has a low ionization energy? Why? 10. Na+ and Mg2+ ions each have ten electrons surrounding their nuclei. Which ion would you expect to have the larger radius? Explain your answer. 11. a. Expl ...
... 9. Is it easier to form a positive ion with an element that has a high ionization energy or an element that has a low ionization energy? Why? 10. Na+ and Mg2+ ions each have ten electrons surrounding their nuclei. Which ion would you expect to have the larger radius? Explain your answer. 11. a. Expl ...
Are there atoms in the air? Why or why not?
... The atomic mass given in the periodic table is an average of the atomic mass of the isotopes of an element. This is because there can be different numbers of neutrons from protons. Scientists will be able to predict where an element falls on the periodic table based on its criteria. ...
... The atomic mass given in the periodic table is an average of the atomic mass of the isotopes of an element. This is because there can be different numbers of neutrons from protons. Scientists will be able to predict where an element falls on the periodic table based on its criteria. ...
Periodic Properties of the Elements
... 3. Record the element’s properties from the list provided in part 1 of Table 1. 4. Note that you can select various periodic trends for the element and period. These trends appear as graphs on the right side of the screen. 5. Observe the graph for atomic radius (pm). Describe the relationship betwee ...
... 3. Record the element’s properties from the list provided in part 1 of Table 1. 4. Note that you can select various periodic trends for the element and period. These trends appear as graphs on the right side of the screen. 5. Observe the graph for atomic radius (pm). Describe the relationship betwee ...
Pretest time!
... levels can attract electrons better (less shielding). So, electronegativity increases UP a group of elements. • In a period: More protons, while the energy levels are the same, means atoms can better attract electrons. So, electronegativity increases RIGHT in a period of elements. ...
... levels can attract electrons better (less shielding). So, electronegativity increases UP a group of elements. • In a period: More protons, while the energy levels are the same, means atoms can better attract electrons. So, electronegativity increases RIGHT in a period of elements. ...
chapter 1 - allenscience
... be titled “Atomic Radius v. Atomic Number”. The top line could be labelled “Group 1: Alkali Metals” and the bottom line could be labeled “Group 18: Noble Gases”. Some students may suggest that all the intervening main-group elements should also be plotted on the graph—an excellent observation, if it ...
... be titled “Atomic Radius v. Atomic Number”. The top line could be labelled “Group 1: Alkali Metals” and the bottom line could be labeled “Group 18: Noble Gases”. Some students may suggest that all the intervening main-group elements should also be plotted on the graph—an excellent observation, if it ...
CP-Chem Ch 5 PowerPoint(The Periodic Table)
... • The extremely low reactivity of noble gases leads to some special uses. ...
... • The extremely low reactivity of noble gases leads to some special uses. ...
Periodic Table Trends - Peoria Public Schools
... Periodic Table Trends Atomic Radii, Ionization Energy, & Electronegativity ...
... Periodic Table Trends Atomic Radii, Ionization Energy, & Electronegativity ...
Periodic Table notes.notebook
... stable, unreactive elements (although some can form compounds), discovered between 1894‐1900, general valence structure ns2np6, general dot diagram, He is the exception ...
... stable, unreactive elements (although some can form compounds), discovered between 1894‐1900, general valence structure ns2np6, general dot diagram, He is the exception ...
Periodic Trends Homework 1) Why does atomic radius decrease as
... electrons to become Be2+ it has the electron configuration of a noble gas (He). This electron configuration is very stable, so a much larger amount of energy is required to remove the third electron. ...
... electrons to become Be2+ it has the electron configuration of a noble gas (He). This electron configuration is very stable, so a much larger amount of energy is required to remove the third electron. ...
Periodic Table Trends
... - Halogens gain electrons easily. - This explains their high reactivity. Group trends: - electron affinity decreases down a group - Electrons add with greater difficulty down a group. ...
... - Halogens gain electrons easily. - This explains their high reactivity. Group trends: - electron affinity decreases down a group - Electrons add with greater difficulty down a group. ...
Periodic data and trends assignment
... b) What happens to the number of energy levels as you move down a column on the periodic table. How and why does this effect ionization energy? The number of energy levels increases by 1 as you move down. This makes the elements have less ionization energy the further you go down, because they have ...
... b) What happens to the number of energy levels as you move down a column on the periodic table. How and why does this effect ionization energy? The number of energy levels increases by 1 as you move down. This makes the elements have less ionization energy the further you go down, because they have ...
the modern periodic law
... chlorine to form colourless compounds which crystallize in cubic shapes and have similar formulas: LiCl, NaCl, KCl, RbCl, CsCl, and FrCl. Halogens are elements of group 17. The word halogen means salt-former. All these elements have non-metallic properties. They react with hydrogen to form compounds ...
... chlorine to form colourless compounds which crystallize in cubic shapes and have similar formulas: LiCl, NaCl, KCl, RbCl, CsCl, and FrCl. Halogens are elements of group 17. The word halogen means salt-former. All these elements have non-metallic properties. They react with hydrogen to form compounds ...
Chapter 5 - EZWebSite
... electrons to the same energy level, but you also add more protons to the nucleus. More protons exerts a stronger attractive force and pulls the electrons in more tightly. What happens to atomic radius as you go down a group? ...
... electrons to the same energy level, but you also add more protons to the nucleus. More protons exerts a stronger attractive force and pulls the electrons in more tightly. What happens to atomic radius as you go down a group? ...
chapter8
... tabulated the elements based on the regular, periodic recurrence of properties. First Mendeleev's classification grouped the elements together more accurately, according to their properties. Mendeleev proposed the existence of an unknown element that he called eka-aluminum. Using data from scatterin ...
... tabulated the elements based on the regular, periodic recurrence of properties. First Mendeleev's classification grouped the elements together more accurately, according to their properties. Mendeleev proposed the existence of an unknown element that he called eka-aluminum. Using data from scatterin ...
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. ...
Chemistry Unit 4: The Periodic Table – Reading
... 10. Where are the lanthanides and actinides located on the table, and why? Section 5.2; pp 138-149 11. Vertical columns are known as ______. What do those elements share in common? 12. Horizontal rows are known as ______. What do those elements share in common? 13. List the name and properties of th ...
... 10. Where are the lanthanides and actinides located on the table, and why? Section 5.2; pp 138-149 11. Vertical columns are known as ______. What do those elements share in common? 12. Horizontal rows are known as ______. What do those elements share in common? 13. List the name and properties of th ...
An element
... • The Periodic table was designed to classify elements according to their properties and to show trends in their physical and chemical properties • The main groups are: I – Alkali metals; II – Alkaline earth metals; VII – Halogens; VIII (also called group ...
... • The Periodic table was designed to classify elements according to their properties and to show trends in their physical and chemical properties • The main groups are: I – Alkali metals; II – Alkaline earth metals; VII – Halogens; VIII (also called group ...
Ch. 6 PPT
... Period: horizontal rows of the Table, show a gradual changing of properties Periodic Law: When elements are arranged in order of increasing Atomic # their properties begin to repeat in a predictable pattern (think Mendeleev) ...
... Period: horizontal rows of the Table, show a gradual changing of properties Periodic Law: When elements are arranged in order of increasing Atomic # their properties begin to repeat in a predictable pattern (think Mendeleev) ...
Chapter 5 The Periodic Table
... configuration for an element in that group. • Def.-an electron that is in the highest occupied energy level of an atom ...
... configuration for an element in that group. • Def.-an electron that is in the highest occupied energy level of an atom ...
Document
... properties – Dmitri first made cards of all the known elements. On each card he wrote the element’s name and all of its properties (e.g. atomic mass, density, color, melting point, and ability to BOND with other elements). The ability to bond with other elements was expressed as VALENCE NUMBER. This ...
... properties – Dmitri first made cards of all the known elements. On each card he wrote the element’s name and all of its properties (e.g. atomic mass, density, color, melting point, and ability to BOND with other elements). The ability to bond with other elements was expressed as VALENCE NUMBER. This ...
2 - HCC Learning Web
... (a) N3− and F− are isoelectronic anions, both containing 10 electrons. Because N3− has only seven protons and F− has nine, the smaller attraction exerted by the nucleus on the electrons results in a larger N3− ion. (b) Both Mg and Ca belong to Group 2A (the alkaline earth metals). Thus, Ca2+ ion is ...
... (a) N3− and F− are isoelectronic anions, both containing 10 electrons. Because N3− has only seven protons and F− has nine, the smaller attraction exerted by the nucleus on the electrons results in a larger N3− ion. (b) Both Mg and Ca belong to Group 2A (the alkaline earth metals). Thus, Ca2+ ion is ...
UNIT 4 NOTES: THE PERIODIC TABLE
... 3. They form _______________ solutions when dissolved in water. For example Cu+2 is ___________, while Fe3+ is ___________. In other words transition elements have _______________ ions. 4. They have _____________________ positive oxidation states. 5. They can ________ electrons from their __________ ...
... 3. They form _______________ solutions when dissolved in water. For example Cu+2 is ___________, while Fe3+ is ___________. In other words transition elements have _______________ ions. 4. They have _____________________ positive oxidation states. 5. They can ________ electrons from their __________ ...
Inorganic Chemistry ELEMENTS AND
... Chemical Bond : Chemical bond may be defined as the attractive force that binds together the constituent atoms in a molecule. Following are some different types of chemical bonds which usually occur in various molecules. (i) Electrovalent bond (Ionic bond) : This type of bond is formed by transfer o ...
... Chemical Bond : Chemical bond may be defined as the attractive force that binds together the constituent atoms in a molecule. Following are some different types of chemical bonds which usually occur in various molecules. (i) Electrovalent bond (Ionic bond) : This type of bond is formed by transfer o ...
Periodicity of Elements and Periodic Table CHAPTER – 4
... 1. They are mono atomic. 2. They exist in gaseous state. 3. Outer most shell of these elements is either complete or contains eight electrons. 4. These elements are mostly chemically non-reactive. 5. These elements have no tendency to form compounds (only a few of these compounds are known). Atomic ...
... 1. They are mono atomic. 2. They exist in gaseous state. 3. Outer most shell of these elements is either complete or contains eight electrons. 4. These elements are mostly chemically non-reactive. 5. These elements have no tendency to form compounds (only a few of these compounds are known). Atomic ...
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.