Molecular Geometry Why?
... is based on the premise that electrons around a central atom repel each other. Electron domains are areas of high electron density such as bonds (single, double or triple) and lone-pairs of electrons. In simple terms VSEPR means that all electron bonding domains and electron nonbonding domains aroun ...
... is based on the premise that electrons around a central atom repel each other. Electron domains are areas of high electron density such as bonds (single, double or triple) and lone-pairs of electrons. In simple terms VSEPR means that all electron bonding domains and electron nonbonding domains aroun ...
Chemistry Review Module Chapter 1
... – Ions are atoms (or clusters of atoms) that have become positively or negatively charged by losing or gaining one or more electrons. Notice the slightly stronger wording with respect to metals than nonmetals! ...
... – Ions are atoms (or clusters of atoms) that have become positively or negatively charged by losing or gaining one or more electrons. Notice the slightly stronger wording with respect to metals than nonmetals! ...
Chapter 30 - The Chemical Basis of Animal Life
... electrons. The second and third shells can each have as many as eight electrons. Larger numbers fill the more distant shells. When the shell of an atom holds the maximum number of electrons possible, the shell is complete and stable. An atom with an incomplete, or unstable, outer shell tends to gain ...
... electrons. The second and third shells can each have as many as eight electrons. Larger numbers fill the more distant shells. When the shell of an atom holds the maximum number of electrons possible, the shell is complete and stable. An atom with an incomplete, or unstable, outer shell tends to gain ...
Atoms, Molecules, and Ions
... community, place on honesty in academic work. The policy defines our expectations for academic honesty and holds students accountable for the integrity of all work they submit. Students should understand that it is their responsibility to learn about course-specific expectations, as well as about un ...
... community, place on honesty in academic work. The policy defines our expectations for academic honesty and holds students accountable for the integrity of all work they submit. Students should understand that it is their responsibility to learn about course-specific expectations, as well as about un ...
General Chemistry Review Problems
... Suppose under perfect conditions the heat transferred should have been 943 cal. Calculate the Percent Error of the experiment in (a). c. How many joules of energy are required to melt a 17 gram ice cube? (The latent heat of fusion of water is 80 cal/g) d. Draw a heating curve for a substance that ha ...
... Suppose under perfect conditions the heat transferred should have been 943 cal. Calculate the Percent Error of the experiment in (a). c. How many joules of energy are required to melt a 17 gram ice cube? (The latent heat of fusion of water is 80 cal/g) d. Draw a heating curve for a substance that ha ...
Name_______________________________________________
... 1. A large difference in electronegativity between two atoms in a bond results in a. polar covalent bonding b. nonpolar covalent bonding c. ionic bonding d. repulsion between two atoms 2. Which of the following happens when atoms bond with each other? a. The atoms increase in potential energy. b. Th ...
... 1. A large difference in electronegativity between two atoms in a bond results in a. polar covalent bonding b. nonpolar covalent bonding c. ionic bonding d. repulsion between two atoms 2. Which of the following happens when atoms bond with each other? a. The atoms increase in potential energy. b. Th ...
Chemical Equation
... • Are compounds composed of charged particles. • In general: the electrons are shared between the ions. Metals tend to give up their electrons to an incomplete nonmetal. • All Ionic compounds are represented by their empirical formulas. They are always in the smallest whole number ratios. ...
... • Are compounds composed of charged particles. • In general: the electrons are shared between the ions. Metals tend to give up their electrons to an incomplete nonmetal. • All Ionic compounds are represented by their empirical formulas. They are always in the smallest whole number ratios. ...
Final Exam - Seattle Central College
... • Know the atomic mass reported on the Periodic Table is the weighted average of all naturally occurring isotopes for that element. • Use the Periodic Table to identify the most abundant isotope of any element given its ...
... • Know the atomic mass reported on the Periodic Table is the weighted average of all naturally occurring isotopes for that element. • Use the Periodic Table to identify the most abundant isotope of any element given its ...
SCSD Physical Science 9th - Shenandoah Community Schools
... Some recognize hydrogen bond (I,D,M) Understand periodic table and periodic trends (I,D,M) o An element is composed of a single type of atom (I,D,M) o Elements are listed in order according to the number of protons (atomic number)(I,D,M) o Repeating patterns of physical and chemical properties ident ...
... Some recognize hydrogen bond (I,D,M) Understand periodic table and periodic trends (I,D,M) o An element is composed of a single type of atom (I,D,M) o Elements are listed in order according to the number of protons (atomic number)(I,D,M) o Repeating patterns of physical and chemical properties ident ...
PowerPoint Presentation - Chapter 2
... Atomic Number and Atomic Mass • Atoms of the various elements differ in number of subatomic particles • An element’s atomic number is the number of protons in its nucleus • An element’s mass number is the sum of protons plus neutrons in the nucleus • Atomic mass, the atom’s total mass, can be appro ...
... Atomic Number and Atomic Mass • Atoms of the various elements differ in number of subatomic particles • An element’s atomic number is the number of protons in its nucleus • An element’s mass number is the sum of protons plus neutrons in the nucleus • Atomic mass, the atom’s total mass, can be appro ...
Examination
... 1 Which statement describes the location of two types of subatomic particles in a helium atom? (1) Protons and neutrons are located in the nucleus. (2) Protons and neutrons are located outside the nucleus. (3) Protons and electrons are located in the nucleus. (4) Protons and electrons are located ou ...
... 1 Which statement describes the location of two types of subatomic particles in a helium atom? (1) Protons and neutrons are located in the nucleus. (2) Protons and neutrons are located outside the nucleus. (3) Protons and electrons are located in the nucleus. (4) Protons and electrons are located ou ...
Electronic Structure and the Periodic Table
... When putting electrons into orbitals with the same energy, place one electron in each orbital before pairing them up. The lone electrons will have the same direction of spin. The existence of unpaired electrons can be tested for ...
... When putting electrons into orbitals with the same energy, place one electron in each orbital before pairing them up. The lone electrons will have the same direction of spin. The existence of unpaired electrons can be tested for ...
Chapter 1.1 –Chemistry is a Physical Science Chemistry is one of
... Chemical properties of matter describe its "potential" to undergo some chemical change or reaction by virtue of its composition. What elements, electrons, and bonding are present to give the potential for chemical change? ...
... Chemical properties of matter describe its "potential" to undergo some chemical change or reaction by virtue of its composition. What elements, electrons, and bonding are present to give the potential for chemical change? ...
Chapter 7
... • These are negatively charged ions resulting from a gain of electrons. • Nonmetals tend to add or share electrons into their highest occupied energy levels to become anions. This allows them to achieve an octet in their highest occupied energy level. • The charge for an anion is written with a numb ...
... • These are negatively charged ions resulting from a gain of electrons. • Nonmetals tend to add or share electrons into their highest occupied energy levels to become anions. This allows them to achieve an octet in their highest occupied energy level. • The charge for an anion is written with a numb ...
summer learning G10
... 4. Jessica heated some bright blue copper(II) nitrate crystals in a test-tube. She noticed brown nitrogen dioxide gas being produced. When a glowing splint was held at the top of the test-tube, it relit, proving that oxygen gas was also produced. A fine black solid, copper(II) oxide, was left in the ...
... 4. Jessica heated some bright blue copper(II) nitrate crystals in a test-tube. She noticed brown nitrogen dioxide gas being produced. When a glowing splint was held at the top of the test-tube, it relit, proving that oxygen gas was also produced. A fine black solid, copper(II) oxide, was left in the ...
end of year review
... _____7. Two compounds that contain the elements carbon and chlorine are carbon tetrachloride (CCl4) and chloroform (CHCl3). Which of the following statements describes the geometry around carbon in these two compounds? A. CCl4 and CHCl3 have bent geometries. B. CCl4 and CHCl3 have tetrahedral geomet ...
... _____7. Two compounds that contain the elements carbon and chlorine are carbon tetrachloride (CCl4) and chloroform (CHCl3). Which of the following statements describes the geometry around carbon in these two compounds? A. CCl4 and CHCl3 have bent geometries. B. CCl4 and CHCl3 have tetrahedral geomet ...
Chemistry Final Test 1999-2000 - Nashoba Valley Technical High
... If element E is a noble gas, which element will form an ion with a -2 oxidation number? A. element A B. element B C. element C D. element D 25) Which of the following correctly describes a trend from top to bottom in the group 1 (1A) elements on the periodic table? A. electronegativity decreases. B. ...
... If element E is a noble gas, which element will form an ion with a -2 oxidation number? A. element A B. element B C. element C D. element D 25) Which of the following correctly describes a trend from top to bottom in the group 1 (1A) elements on the periodic table? A. electronegativity decreases. B. ...
Electrons
... Atomic Number and Atomic Mass • Atoms of the various elements differ in number of subatomic particles • An element’s atomic number is the number of protons in its nucleus • An element’s mass number is the sum of protons plus neutrons in the nucleus • Atomic mass, the atom’s total mass, can be appro ...
... Atomic Number and Atomic Mass • Atoms of the various elements differ in number of subatomic particles • An element’s atomic number is the number of protons in its nucleus • An element’s mass number is the sum of protons plus neutrons in the nucleus • Atomic mass, the atom’s total mass, can be appro ...
Chemistry 515 Name: L. S. Curtin Soc. Sec. #: February 8, 1999
... a) The number of protons and neutrons in the nucleus of an atom are always equal. b) The mass of an atom is contained primarily in the nucleus and the volume of an atom is primarily determined by the size of the electron cloud. c) Isotopes of a given element have very different chemical reactivities ...
... a) The number of protons and neutrons in the nucleus of an atom are always equal. b) The mass of an atom is contained primarily in the nucleus and the volume of an atom is primarily determined by the size of the electron cloud. c) Isotopes of a given element have very different chemical reactivities ...
9077590 Chem. Rege. Jan. 01
... This part consists of twelve groups, each containing five questions. Each group tests a major area of the course. Choose seven of these twelve groups. Be sure that you answer all five questions in each group chosen. Record the answers to these questions on the separate answer sheet in accordance wit ...
... This part consists of twelve groups, each containing five questions. Each group tests a major area of the course. Choose seven of these twelve groups. Be sure that you answer all five questions in each group chosen. Record the answers to these questions on the separate answer sheet in accordance wit ...
Metals
... •Ordered elements by atomic mass •Repeating pattern of properties •Elements with similar properties in the same column Periodic Law – when the elements are arranged in order of increasing atomic mass, certain sets of ...
... •Ordered elements by atomic mass •Repeating pattern of properties •Elements with similar properties in the same column Periodic Law – when the elements are arranged in order of increasing atomic mass, certain sets of ...
Chemistry A - Montgomery County Public Schools
... describe the characteristics of protons, neutrons and electrons in terms of location, charge and mass. illustrate the structure of the atom by using the Bohr model, including the charge, relative mass and location of the sub-atomic particles. use atomic mass, atomic number, and charge to ident ...
... describe the characteristics of protons, neutrons and electrons in terms of location, charge and mass. illustrate the structure of the atom by using the Bohr model, including the charge, relative mass and location of the sub-atomic particles. use atomic mass, atomic number, and charge to ident ...
2 - FacultyWeb
... • A hydrogen bond forms when a hydrogen atom covalently bonded to one electronegative atom is also attracted to another electronegative atom In living cells, the electronegative partners of hydrogen are usually oxygen or nitrogen atoms • Hydrogen bonds are common between dipoles such as water • Hy ...
... • A hydrogen bond forms when a hydrogen atom covalently bonded to one electronegative atom is also attracted to another electronegative atom In living cells, the electronegative partners of hydrogen are usually oxygen or nitrogen atoms • Hydrogen bonds are common between dipoles such as water • Hy ...
Chapter 2 PowerPoint
... Strategy Note that the compounds in (a) and (b) contain both metal and nonmetal atoms, so we expect them to be ionic compounds. There are no metal atoms in (c) but there is an ammonium group, which bears a positive charge. So NH 4ClO3 is also an ionic compound. Our reference for the names of cations ...
... Strategy Note that the compounds in (a) and (b) contain both metal and nonmetal atoms, so we expect them to be ionic compounds. There are no metal atoms in (c) but there is an ammonium group, which bears a positive charge. So NH 4ClO3 is also an ionic compound. Our reference for the names of cations ...
Atoms, Molecules and Ions - Moodle @ FCT-UNL
... Strategy Note that the compounds in (a) and (b) contain both metal and nonmetal atoms, so we expect them to be ionic compounds. There are no metal atoms in (c) but there is an ammonium group, which bears a positive charge. So NH4ClO3 is also an ionic compound. Our reference for the names of cations ...
... Strategy Note that the compounds in (a) and (b) contain both metal and nonmetal atoms, so we expect them to be ionic compounds. There are no metal atoms in (c) but there is an ammonium group, which bears a positive charge. So NH4ClO3 is also an ionic compound. Our reference for the names of cations ...
Electronegativity
Electronegativity, symbol χ, is a chemical property that describes the tendency of an atom or a functional group to attract electrons (or electron density) towards itself. An atom's electronegativity is affected by both its atomic number and the distance at which its valence electrons reside from the charged nucleus. The higher the associated electronegativity number, the more an element or compound attracts electrons towards it. The term ""electronegativity"" was introduced by Jöns Jacob Berzelius in 1811,though the concept was known even before that and was studied by many chemists including Avogadro.In spite of its long history, an accurate scale of electronegativity had to wait till 1932, when Linus Pauling proposed an electronegativity scale, which depends on bond energies, as a development of valence bond theory. It has been shown to correlate with a number of other chemical properties. Electronegativity cannot be directly measured and must be calculated from other atomic or molecular properties. Several methods of calculation have been proposed, and although there may be small differences in the numerical values of the electronegativity, all methods show the same periodic trends between elements. The most commonly used method of calculation is that originally proposed by Linus Pauling. This gives a dimensionless quantity, commonly referred to as the Pauling scale, on a relative scale running from around 0.7 to 3.98 (hydrogen = 2.20). When other methods of calculation are used, it is conventional (although not obligatory) to quote the results on a scale that covers the same range of numerical values: this is known as an electronegativity in Pauling units. As it is usually calculated, electronegativity is not a property of an atom alone, but rather a property of an atom in a molecule. Properties of a free atom include ionization energy and electron affinity. It is to be expected that the electronegativity of an element will vary with its chemical environment, but it is usually considered to be a transferable property, that is to say that similar values will be valid in a variety of situations.On the most basic level, electronegativity is determined by factors like the nuclear charge (the more protons an atom has, the more ""pull"" it will have on electrons) and the number/location of other electrons present in the atomic shells (the more electrons an atom has, the farther from the nucleus the valence electrons will be, and as a result the less positive charge they will experience—both because of their increased distance from the nucleus, and because the other electrons in the lower energy core orbitals will act to shield the valence electrons from the positively charged nucleus).The opposite of electronegativity is electropositivity: a measure of an element's ability to donate electrons.Caesium is the least electronegative element in the periodic table (=0.79), while fluorine is most electronegative (=3.98). (Francium and caesium were originally assigned both assigned 0.7; caesium's value was later refined to 0.79, but no experimental data allows a similar refinement for francium. However, francium's ionization energy is known to be slightly higher than caesium's, in accordance with the relativistic stabilization of the 7s orbital, and this in turn implies that caesium is in fact more electronegative than francium.)