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Fall Exam 3
... An atomic orbital describes the three-dimensional distribution of an electron in space as defined by a set of quantum numbers. An orbital describes the circular orbit that an electron follows around the nucleus. Superimposing the electron density in a filled set of s, p and d orbitals results in a c ...
... An atomic orbital describes the three-dimensional distribution of an electron in space as defined by a set of quantum numbers. An orbital describes the circular orbit that an electron follows around the nucleus. Superimposing the electron density in a filled set of s, p and d orbitals results in a c ...
Notes
... Compounds are formed when atoms of elements combine. Law of constant composition: The relative kinds and numbers of atoms are constant for a given compound. Law of conservation of mass (matter): During a chemical reaction, the total mass before the reaction is equal to the total mass after the rea ...
... Compounds are formed when atoms of elements combine. Law of constant composition: The relative kinds and numbers of atoms are constant for a given compound. Law of conservation of mass (matter): During a chemical reaction, the total mass before the reaction is equal to the total mass after the rea ...
Chpt. 5 Study Guide for Fall Final
... E) None of the above 8) Which statement is true about the discovery of electrons? A) Electrons were discovered after the TV tube was invented. B ) Electrons were discovered when anode rays were identified in an anode ray tube. C) Electrons were discovered by experimental chemists. D) Electrons were ...
... E) None of the above 8) Which statement is true about the discovery of electrons? A) Electrons were discovered after the TV tube was invented. B ) Electrons were discovered when anode rays were identified in an anode ray tube. C) Electrons were discovered by experimental chemists. D) Electrons were ...
Chapter 1 The Periodic Table - Beck-Shop
... Atoms have a central nucleus surrounded by orbiting electrons. Electrons exist in energy levels called shells. Each shell can hold a certain maximum number of electrons. Shells are subdivided into energy levels called subshells. ...
... Atoms have a central nucleus surrounded by orbiting electrons. Electrons exist in energy levels called shells. Each shell can hold a certain maximum number of electrons. Shells are subdivided into energy levels called subshells. ...
WHAT IS THE BASIC STRUCTURE OF THE ATOM
... 5. The atomic masses of the elements are listed on the periodic table, but they are not whole numbers. 6. This is because the _______________ of an element is the weighted average mass of that element. 7. Weighted averages depend on two factors: the __________ and the ____________________ of each ...
... 5. The atomic masses of the elements are listed on the periodic table, but they are not whole numbers. 6. This is because the _______________ of an element is the weighted average mass of that element. 7. Weighted averages depend on two factors: the __________ and the ____________________ of each ...
9April2012 Notes
... atomic # from it. (11) A mole is a unit of quantity. It is equal to Avogadro’s Number which is 6.022 x 1023 atoms or molecules or particles. Because each element has a different # of protons & neutrons, each will have a different molar mass (another name for the “weighted average mass”). For instanc ...
... atomic # from it. (11) A mole is a unit of quantity. It is equal to Avogadro’s Number which is 6.022 x 1023 atoms or molecules or particles. Because each element has a different # of protons & neutrons, each will have a different molar mass (another name for the “weighted average mass”). For instanc ...
Unit B: Matter and Chemical Change
... Note: The hydrogen atom has the atomic number of 1 therefore contains 1 electron. This electron is found in the first orbital and has room to gain 1 more electron if it comes in contact with another atom. This would then completely fill the first orbital. Nitrogen’s atom has the atomic number of 7 ...
... Note: The hydrogen atom has the atomic number of 1 therefore contains 1 electron. This electron is found in the first orbital and has room to gain 1 more electron if it comes in contact with another atom. This would then completely fill the first orbital. Nitrogen’s atom has the atomic number of 7 ...
SECTION 3-2: THE STRUCTURE OF THE ATOM
... 1. Nucleus: * Has at least one positively charged particle called a proton and generally one or more neutral particles called neutrons. * Very small region located near the center of the atom 2. Electrons: Surrounds the nucleus (electron cloud) and are negatively charged Protons, neutrons, and elect ...
... 1. Nucleus: * Has at least one positively charged particle called a proton and generally one or more neutral particles called neutrons. * Very small region located near the center of the atom 2. Electrons: Surrounds the nucleus (electron cloud) and are negatively charged Protons, neutrons, and elect ...
Atomic Theory
... Expected result: particles would pass through Actual result: most passed through, but some were deflected and reflected These results indicated a concentration of positive charge (nucleus), with electrons moving around it at some distance. ...
... Expected result: particles would pass through Actual result: most passed through, but some were deflected and reflected These results indicated a concentration of positive charge (nucleus), with electrons moving around it at some distance. ...
atoms - My CCSD
... identical. Atoms of any one element are different from those of any other element. ...
... identical. Atoms of any one element are different from those of any other element. ...
PERIODIC TABLE OF THE ELEMENTS
... • Transition metals are usually shiny. – E.g. silver (Ag), gold (Au), and platinum (Pt) ...
... • Transition metals are usually shiny. – E.g. silver (Ag), gold (Au), and platinum (Pt) ...
Atoms and the Periodic Table
... rule. All atoms want to have eight electrons or complete orbitals in their highest energy level. Add or take away electrons according to this rule. ...
... rule. All atoms want to have eight electrons or complete orbitals in their highest energy level. Add or take away electrons according to this rule. ...
Atomic Structure
... • 1. All elements are composed of tiny indivisible particles called atoms. • 2. Atoms of the same element are identical. The atoms of one element are different from the atoms of another element. • 3. Atoms of different elements can physically mix together or can chemically combine in simplewhole num ...
... • 1. All elements are composed of tiny indivisible particles called atoms. • 2. Atoms of the same element are identical. The atoms of one element are different from the atoms of another element. • 3. Atoms of different elements can physically mix together or can chemically combine in simplewhole num ...
can be determined without changing the identity of matter
... SUBSTANCES - CANNOT be separated into different materials by PHYSICAL PROCESSES Examples: Table salt, gold, silver, nitrogen, oxygen, carbon, hydrochloric acid, carbon dioxide, ethanol (grain alcohol), water, silicon dioxide ...
... SUBSTANCES - CANNOT be separated into different materials by PHYSICAL PROCESSES Examples: Table salt, gold, silver, nitrogen, oxygen, carbon, hydrochloric acid, carbon dioxide, ethanol (grain alcohol), water, silicon dioxide ...
AP Semester I Review: Free Response Questions
... The structures of a water molecule and a crystal of LiCl(s) are represented above. A student prepares a 1.0 M solution by dissolving 4.2 g of LiCl(s) in enough water to make 100 mL of solution. a. In the space provided below, show the interactions of the components of LiCl(aq) by making a drawing th ...
... The structures of a water molecule and a crystal of LiCl(s) are represented above. A student prepares a 1.0 M solution by dissolving 4.2 g of LiCl(s) in enough water to make 100 mL of solution. a. In the space provided below, show the interactions of the components of LiCl(aq) by making a drawing th ...
Document
... A) alkali metals have the lowest ionization energy B) alkali metals have the highest ionization energy C) halogens metals have the lowest ionization energy D) inert gases metals have the lowest ionization energy ...
... A) alkali metals have the lowest ionization energy B) alkali metals have the highest ionization energy C) halogens metals have the lowest ionization energy D) inert gases metals have the lowest ionization energy ...
the atom
... An element when composed of one type of atom, and canNOT be broken down chemically into simpler substances. Hydrogen and oxygen are examples of elements. A compound when composed of two or more types of elements combined in a definite ratio, and can be decomposed by a chemical change into two or mor ...
... An element when composed of one type of atom, and canNOT be broken down chemically into simpler substances. Hydrogen and oxygen are examples of elements. A compound when composed of two or more types of elements combined in a definite ratio, and can be decomposed by a chemical change into two or mor ...
Chemistrypart107
... • 1. If protons and electrons do not match, then it is an ion. • 2. If protons and neutrons do not match the atomic mass (number below element symbol) of element then it an isotope. • 3. If protons and electrons match, neutrons and protons = atomic mass # then the element is stable ...
... • 1. If protons and electrons do not match, then it is an ion. • 2. If protons and neutrons do not match the atomic mass (number below element symbol) of element then it an isotope. • 3. If protons and electrons match, neutrons and protons = atomic mass # then the element is stable ...
SCIENCE LONG TEST
... 2. Covalent bonding – sharing of electrons; both non metals 1. Hydrogen – prone to covalent bonding 2. Gilbert Lewis reasoned out that atoms could also obtain noble gas electron configurations by sharing their electrons 3. No one gains/loses electrons 4. The bonding pair of electrons is usually sho ...
... 2. Covalent bonding – sharing of electrons; both non metals 1. Hydrogen – prone to covalent bonding 2. Gilbert Lewis reasoned out that atoms could also obtain noble gas electron configurations by sharing their electrons 3. No one gains/loses electrons 4. The bonding pair of electrons is usually sho ...
6.5 Main Group
... Inert Pair effect: Although the ionization energy decreases down the group with increasing atomic radius (heavier elements form cations more readily), the heavier elements also show greater stability of M+ (ns2np0). One possible explanation is that the ns2 electrons are harder to remove due to a rel ...
... Inert Pair effect: Although the ionization energy decreases down the group with increasing atomic radius (heavier elements form cations more readily), the heavier elements also show greater stability of M+ (ns2np0). One possible explanation is that the ns2 electrons are harder to remove due to a rel ...
chapter5 - MrFoti.com
... Counting the Pieces Atomic Number = number of protons in the nucleus # of protons determines kind of atom (since all protons are alike!) the same as the number of electrons in the neutral atom. Mass Number = the number of protons + neutrons in a particular isotope of that element. These acc ...
... Counting the Pieces Atomic Number = number of protons in the nucleus # of protons determines kind of atom (since all protons are alike!) the same as the number of electrons in the neutral atom. Mass Number = the number of protons + neutrons in a particular isotope of that element. These acc ...
Periodic table
The periodic table is a tabular arrangement of the chemical elements, ordered by their atomic number (number of protons in the nucleus), electron configurations, and recurring chemical properties. The table also shows four rectangular blocks: s-, p- d- and f-block. In general, within one row (period) the elements are metals on the lefthand side, and non-metals on the righthand side.The rows of the table are called periods; the columns are called groups. Six groups (columns) have names as well as numbers: for example, group 17 elements are the halogens; and group 18, the noble gases. The periodic table can be used to derive relationships between the properties of the elements, and predict the properties of new elements yet to be discovered or synthesized. The periodic table provides a useful framework for analyzing chemical behavior, and is widely used in chemistry and other sciences.Although precursors exist, Dmitri Mendeleev is generally credited with the publication, in 1869, of the first widely recognized periodic table. He developed his table to illustrate periodic trends in the properties of the then-known elements. Mendeleev also predicted some properties of then-unknown elements that would be expected to fill gaps in this table. Most of his predictions were proved correct when the elements in question were subsequently discovered. Mendeleev's periodic table has since been expanded and refined with the discovery or synthesis of further new elements and the development of new theoretical models to explain chemical behavior.All elements from atomic numbers 1 (hydrogen) to 118 (ununoctium) have been discovered or reportedly synthesized, with elements 113, 115, 117, and 118 having yet to be confirmed. The first 94 elements exist naturally, although some are found only in trace amounts and were synthesized in laboratories before being found in nature. Elements with atomic numbers from 95 to 118 have only been synthesized in laboratories. It has been shown that einsteinium and fermium once occurred in nature but currently do not. Synthesis of elements having higher atomic numbers is being pursued. Numerous synthetic radionuclides of naturally occurring elements have also been produced in laboratories.