Polar and Nonpolar Covalent Compounds
... IPC - Mr. Coburn Introduction The tendency of an atom to attract electrons is called electronegativity. Atoms of elements that have higher electronegativities "pull" the electrons toward them with more force. Ionic chemical bonds are formed between oppositely charged ions when valence electrons are ...
... IPC - Mr. Coburn Introduction The tendency of an atom to attract electrons is called electronegativity. Atoms of elements that have higher electronegativities "pull" the electrons toward them with more force. Ionic chemical bonds are formed between oppositely charged ions when valence electrons are ...
Units 3 and 4 Revision
... These elements have the same number of electrons in their outer energy level – this gives them similar properties. Q10. Chlorine atoms exists as two different isotopes 35Cl and 37Cl. ...
... These elements have the same number of electrons in their outer energy level – this gives them similar properties. Q10. Chlorine atoms exists as two different isotopes 35Cl and 37Cl. ...
Labs - newtunings.com
... 3.4f The rate of a chemical reaction depends on several factors: temperature, concentration, nature of the reactants, surface area, and the presence of a catalyst. 3.4g A catalyst provides an alternate reaction pathway, which has a lower activation energy than an uncatalyzed reaction. 3.4h Some chem ...
... 3.4f The rate of a chemical reaction depends on several factors: temperature, concentration, nature of the reactants, surface area, and the presence of a catalyst. 3.4g A catalyst provides an alternate reaction pathway, which has a lower activation energy than an uncatalyzed reaction. 3.4h Some chem ...
Chemistry Semester One Exam Review Name:
... 5. Distinguish the symbols of common elements, and match the names of common elements to their symbols a. Aluminum – ...
... 5. Distinguish the symbols of common elements, and match the names of common elements to their symbols a. Aluminum – ...
- Catalyst
... Question 7: Fill in the blanks of the statements below with the words in the box. Note, you will only use each word once. A. atom ...
... Question 7: Fill in the blanks of the statements below with the words in the box. Note, you will only use each word once. A. atom ...
Chemical Bonds - coellochemistry
... nonmetals must have prefixes assigned to represent the number of atoms The second element has a prefix and has the ending changed to -ide ...
... nonmetals must have prefixes assigned to represent the number of atoms The second element has a prefix and has the ending changed to -ide ...
No Slide Title
... Comparison of Group 1A and 1B The metals in these two groups have similar outer electron configurations, with one electron in the outermost s orbital. Chemical properties are quite different due to difference in the ionization energy. ...
... Comparison of Group 1A and 1B The metals in these two groups have similar outer electron configurations, with one electron in the outermost s orbital. Chemical properties are quite different due to difference in the ionization energy. ...
1.5.16(Chem) - mrcarlsonschemistryclass
... Cations and Anions • Cations are ions with a POSITIVE charge. • Anions are ions with a NEGATIVE charge. • Draw the funny way to remember cations and anions: ...
... Cations and Anions • Cations are ions with a POSITIVE charge. • Anions are ions with a NEGATIVE charge. • Draw the funny way to remember cations and anions: ...
Final Exam Review
... 67. Which of the following compounds are most likely not ionic? A. H2O B. Na2O C. CO2 D. CaS E. SO2 F. NH3 ...
... 67. Which of the following compounds are most likely not ionic? A. H2O B. Na2O C. CO2 D. CaS E. SO2 F. NH3 ...
4 - College of Arts and Sciences
... Identify the GROUP of elements that corresponds to each of the following generalized electron configurations ...
... Identify the GROUP of elements that corresponds to each of the following generalized electron configurations ...
Outline Chapter 10 The Periodic Law
... Periodic law=states that when elements are listed in order of atomic number, elements with similar chemical and physical properties appear at regular intervals. Periodic table = listing of elements according to atomic number in a series of rows such that elements with similar properties form vertica ...
... Periodic law=states that when elements are listed in order of atomic number, elements with similar chemical and physical properties appear at regular intervals. Periodic table = listing of elements according to atomic number in a series of rows such that elements with similar properties form vertica ...
CHEMISTRY FINAL EXAM REVIEW SHEET
... Proton: +1 charge, located in nucleus, relative mass = 1 amu Neutron: No charge, located in nucleus, relative mass = 1 amu Electron: -1 charge, located outside of nucleus, relative mass = 1/1840 amu Atomic Number = number of protons in an element. Mass Number = number of protons + neutrons in an ele ...
... Proton: +1 charge, located in nucleus, relative mass = 1 amu Neutron: No charge, located in nucleus, relative mass = 1 amu Electron: -1 charge, located outside of nucleus, relative mass = 1/1840 amu Atomic Number = number of protons in an element. Mass Number = number of protons + neutrons in an ele ...
Name: Midterm Review (Part II) Fill in the blanks (Chapter 6.1 – 6.3
... How do nonmetals obey the octet rule when reacting to form ionic compounds? How do nonmetals obey the octet rule when reacting to form covalent compounds? How many valence electrons there are in S-2 ion? S-2 anion has a larger/smaller radius than a neutral Sulfur (S) atom. A covalent bond is a bond ...
... How do nonmetals obey the octet rule when reacting to form ionic compounds? How do nonmetals obey the octet rule when reacting to form covalent compounds? How many valence electrons there are in S-2 ion? S-2 anion has a larger/smaller radius than a neutral Sulfur (S) atom. A covalent bond is a bond ...
Reactions I Can..
... the relative mass composition of the constituent elements. 10. Calculate the molecular formula of a compound given the empirical formula and the molecular mass. 11. Summarize how the gas variables of P, V, n, And T relate to each other in common situations such as the air in a car tire or the air in ...
... the relative mass composition of the constituent elements. 10. Calculate the molecular formula of a compound given the empirical formula and the molecular mass. 11. Summarize how the gas variables of P, V, n, And T relate to each other in common situations such as the air in a car tire or the air in ...
Atoms
... metals, alkaline earth metals, halogens, noble gases, lanthanide series, actinide series, transition elements, inner-transition elements, and trans-uranic elements. 6. Identify the phase (solid, liquid, gas) of each element on the Periodic Table. 7. Explain the basic periodic trends of radius and io ...
... metals, alkaline earth metals, halogens, noble gases, lanthanide series, actinide series, transition elements, inner-transition elements, and trans-uranic elements. 6. Identify the phase (solid, liquid, gas) of each element on the Periodic Table. 7. Explain the basic periodic trends of radius and io ...
Midterm Review File
... 25. If an atom has an electron configuration of 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2, how many valence electrons does it have? ...
... 25. If an atom has an electron configuration of 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2, how many valence electrons does it have? ...
Chemistry Test Review - Greenslime Home Page
... a. Atom – the smallest part of an element that still acts like that element; can’t be broken down; basic part of matter b. Element – a substance that cannot be broken down into simpler substances containing only 1 type of atom c. Compound – two or more different elements chemically combined d. Molec ...
... a. Atom – the smallest part of an element that still acts like that element; can’t be broken down; basic part of matter b. Element – a substance that cannot be broken down into simpler substances containing only 1 type of atom c. Compound – two or more different elements chemically combined d. Molec ...
Dr. Harris Chemistry 105 Practice Exam 1 Isotope Atomic Number
... 6. Answer the following. a.) Using electron configurations, show the formation of MgO. b.) Why does this reaction proceed? (3) ...
... 6. Answer the following. a.) Using electron configurations, show the formation of MgO. b.) Why does this reaction proceed? (3) ...
Document
... 10. How many Chlorine atoms are present in the compound Ca(ClO3)2? 11. How many hydrogen atoms are present in one molecule of ammonium acetate, NH4C2H3O2? 12. What is the name of the compound with the formula NaCl? 13. Why do the noble gases NOT form compounds readily? 14. In a chemical formula, the ...
... 10. How many Chlorine atoms are present in the compound Ca(ClO3)2? 11. How many hydrogen atoms are present in one molecule of ammonium acetate, NH4C2H3O2? 12. What is the name of the compound with the formula NaCl? 13. Why do the noble gases NOT form compounds readily? 14. In a chemical formula, the ...
How are Molecules Depicted? - Belle Vernon Area School District
... which e- are represented by dots: dot pairs or dashes b/t 2 atomic symbols represents pairs in covalent bonds ...
... which e- are represented by dots: dot pairs or dashes b/t 2 atomic symbols represents pairs in covalent bonds ...
Chemical Bonding I: Lewis Theory
... • Very good at showing what can and cannot form! • Predicts directionality. • Works very well with organic compounds. • Exceptions are interesting and will be discussed later! ...
... • Very good at showing what can and cannot form! • Predicts directionality. • Works very well with organic compounds. • Exceptions are interesting and will be discussed later! ...
document
... breaks down into its parts. 2. Ion C B. A bond that is formed by sharing electrons. 3. Charge D C. A charged atom. D. The number of electrons an 4. Covalent Bond B element is willing to gain, lose, or share to form compounds. 5. Ionic Bond I E. States that all elements want either a full outer shell ...
... breaks down into its parts. 2. Ion C B. A bond that is formed by sharing electrons. 3. Charge D C. A charged atom. D. The number of electrons an 4. Covalent Bond B element is willing to gain, lose, or share to form compounds. 5. Ionic Bond I E. States that all elements want either a full outer shell ...
Atomic Structure: SOL Review #1 Name: Historical Developments 1
... The electrons are not “singly before pairing.” Electrons repel each other, so they do want not pair until there is no more “space” left in the sublevel. Periodic Table and Periodic Trends 27) Which elements would have similar properties to Na? ...
... The electrons are not “singly before pairing.” Electrons repel each other, so they do want not pair until there is no more “space” left in the sublevel. Periodic Table and Periodic Trends 27) Which elements would have similar properties to Na? ...
Chemistry Midterm Review 2006
... allows us to observe flame tests? c. Is energy released or absorbed when an electron falls from a higher energy level to a lower energy level? 7. What is the difference between a ground state and an excited state? 8. What is the lowest energy level? The lowest sublevel? 9. What is the maximum number ...
... allows us to observe flame tests? c. Is energy released or absorbed when an electron falls from a higher energy level to a lower energy level? 7. What is the difference between a ground state and an excited state? 8. What is the lowest energy level? The lowest sublevel? 9. What is the maximum number ...
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.)