The center-most part of an atom where the protons and neutrons 5. The weighted average mass of an element’s isotopes of that element 4. The smallest particle of an element that retains the properties 3. High-energy radiation that has no charge and no mass of neutrons 2. Atoms with the same number of protons but different numbers 1.
2) Define weighted average- An average that takes into account the proportional relevance of each component, rather than treating each component equally. 3) Place one atom of each isotope on the scale. Divide the mass by 3 to fine the straight average. How is this number different from your average atomic mass? Number – 19g average mass 1.7g 4) If a 4th isotope of beanium, D (green), were added to the pool, how would the average atomic mass change?
Neutrons, Protons and electrons are all sub-atomic particles. In relative mass, we always think of protons and neutrons in having a mass of 1 and electrons a mass of 1/1840, which shows that electrons are considerably smaller than protons and neutrons, and only make up a small part of the atom. The amount of protons and neutrons added together is the relative atomic mass, and this is the main structure of the atom. 2. The arrangement of particles in an atom Protons and neutrons make up the main, dense, central nucleus in the centre of the atom.
Nuclear fussion: Nuclear fusion is the process in which two light nuclei combine to form a heavier nucleus. The total masses of the products are less than the combined mass of the two light nuclei. The energy equivalent of the loss of mass is released. The release of energy during nuclear fusion can also be calculated from the values of the
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.
(Divide the mass of the solid by the volume of the solid calculated above.) Trial 1: 41.256 / .5 = 82.512 Trial 2: 42.299 / .5 = 84.598 Trial 3: 40.462 / .4 = 101.155 Part III: Density of Regular-Shaped Solid Calculate the volume of the regular shaped solid for each trial. (Multiply the length × width × height for each trial to get the volume in the unit cm3.) Trial 1: 5.3 x 3 x 2.5 = 39.75 Trial 2: 5 x 4 x 3 = 60 Trial 3: 4.5 x 3.5 x 2 = 31.5 Calculate the density of the regular-shaped solid for each trial. (Divide the mass of the solid by the volume calculated above.)
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.
Which one of the following molecules has tetrahedral geometry? A. CF4 B. XeF4 C. BF3 D. NH3 E. AsF5 63. A molecule with 3 single bonds and 0 lone pairs of electrons is predicted to have which type of molecular geometry? A. Trigonal planar B. Trigonal pyramidal C. Bent D. Trigonal bipyramidal E. Linear 64. A central atom with 4 electron pairs (single bonds and/or lone pairs of electrons) could have which of the following molecular geometries?
Structure of living organisms Living organisms are made up of quarks, sub-atomic particles, atoms, molecules, cells, tissues, organs and organ systems. A quark is a basic particle and a important component of matter. Quarks combine to form compound particles called hadrons, the most stable of which are protons and neutrons, the components of atomic nuclei. There are six types of quarks, known as flavors: up, down, strange, charm, bottom, and top. Up and down quarks have the lowest masses of all quarks.