Name___________________________ Period_________________ Chemical Bonds Review Sheet Part one Write the definitions for each of the following terms. Octet rule Cation Anion Ionic compound Monatomic ion Covalent bond Molecular compound Nonpolar covalent bond Polar covalent bond Single bond Double bond Triple bond Part 2 1. Which has a greater potential energy, a noble gas or a metal? Explain your answer. ________________________________________________________________ ________________________________________________________________ ________________________________________________________________ 2.
Test #2 ANSWERS CHM 101 Part I Multiple Choice (2 points each) 1. Which element is most likely to form three covalent bonds? A) C B) Si C) P D) S E) Se 2. A chemical bond formed when two atoms share two pairs of electrons is a ________ bond; it is best described as ________. A) double; covalent B) double; ionic C) single; covalent D) single; ionic E) triple; covalent 3.
Energy levels and electron configurations (including representation using orbital diagrams) of several common elements on the periodic table. Identify groups and periods of elements on the periodic table, and know the trends of reactivity, atomic size, ionization energy, and electron affinity within a group or period. Page 297 - 320; page 325 – 329; page 341 – 350 and page 353 – 359; page 393 – 420; * Chemical bonding and Lewis structures. Molecular geometry. Gases (concepts and problem
N05/4/PHYSI/SPM/ENG/TZ0/XX+ The mass of an atom of the isotope strontium-92 (92Sr) is of the order of A. B. C. D. 10–23 kg. 10–25 kg. 10–27 kg. 10–29 kg.
C, c. H, d. Fe, e. N, f. 0, g. K, h. Na (p. 29) 26. a. All three are carbon with six protons. (p. 30) b. All possess different numbers of neutrons and therefore have different atomic masses. (p. 31) c.
Explain your reasoning. * An atom of Y would be smaller than X because the ionization levels are larger than X. The electrons of Y are bound to the nucleus stronger than the X electrons. 8.30. Periodic Properties II Consider two hypothetical elements, W and Z.
4Below is the high resolution 1H NMR spectrum of Compound G [pic] This compound contains C, H and N atoms. 1 How many peaks are there in the first signal (past the TMS from the right) and what can be concluded from this? 1½ marks 2 How many peaks has the second signal split into, and what can be concluded from this? 1½ marks 3 Determine the semi-structural formula of compound G and name the compound. 2 marks 4 Draw the structural formula of Compound G. 1 mark 5 Using the chemical shift correlation for 13C NMR, predict the number of peaks for Compound G and draw in the position of the peaks on the blank spectrum below, annotating each peak with its corresponding structure.
OCR B CHEMISTRY F331 (Unit 1) Revision Guide 2014 Formulae, equations and amount of substance | Key Terms (a). * Atomic Number: Atomic number is the number of protons in the nucleus. * Mass Number: Mass number is defined as the sum of the numbers of protons and neutrons in the atom’s nucleus. * Isotopes: Atoms with the same number of protons but different number of neutrons are called isotopes; they therefore have different masses. * Avogadro’s constant: The number of toms per mole is called the Avogadro’s constant.
Describe the differences between protons and electrons The difference between protons and electrons is that protons are positively charged and that elections are negatively charged. Another difference is that protons are in the nucleus and electrons circle the nucleus in shells outside the nucleus. What is the difference between the mass number and the relative atomic mass of an element? The difference between the mass number and the atomic mass is that the mass number is the number of protons and neutrons in the nucleus and the relative atomic mass is the mass of an atom. Distinguish between an element and a compound with 2 examples for each An element is a substance that cannot be broken down into any simpler substances.
David Kemp OCR Chemistry A Unit 1: F321 Atomic Structure (a) describe protons, neutrons and electrons in terms of relative charge and relative mass; Proton +1 1 Neutron 0 1 Electron -1 1/2000 Relative Charge Relative Mass (b) describe the distribution of mass and charge Within an atom; Positively charged Nucleus containing most of the mass, surrounded by atomic shells with orbiting electrons of negative charge and negligible mass. (c) describe the contribution of protons and neutrons to the nucleus of an atom, in terms of atomic (proton) number and mass (nucleon) number. The atomic number of the nucleus, also the proton number, shows the number of protons in the nucleus. It also defines the element. The number of neutrons added to the number of protons is the nucleon number or mass number.