Chapter 2 - Stable for Life
Chapter 2 - Stable for Life A104
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This 6 page Class Notes was uploaded by KUMIKO Notetaker on Saturday September 19, 2015. The Class Notes belongs to A104 at Republic Polytechnic taught by Lynette Liaw in Summer 2015. Since its upload, it has received 44 views. For similar materials see Biology in Applied Science at Republic Polytechnic.
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Date Created: 09/19/15
ghapter 2 Stable for Life Atoms Basic building blocks of matter Electrically neutral The number of protons and electrons is the same in an atom Centre of an atom is the nucleus Composed of protons neutrons and electrons Protons are positively charged particles Electrons are negatively charged particles and reside in shells surrounding the nucleus Neutrons do not carry any charge Practice Questions 1 1 List down some information that you know about atoms 2 Based on your understanding of the subatomic particles determine the charges of the following a Proton b Neutron c Electron 2 Why the electrons are able to remain in the region around the nucleus 3 All atoms are electrically neutral a Discuss what you understand by the term 39electrically neutral39 b Give a reason for the statement Electron Shell Diagram 0 Each electron shell is associated with xed energy level and can hold a xed number of electrons The occupied shell furthest away from the nucleus is known as the valence shell with electrons residing in it de ned as valence electrons Ellery aidsnen Maximum 18 e Endshel l Maximum e 1513mm Maximum e Practice Questions 2 1 Electrons revolve along imaginary paths around the nucleus known as shells a True b False 2 Suggest why electrons in an atom can remain in the region around its nucleus 3 When increasing the electron shell the energy level will be decreased a True b False 2 How many electrons does the a valence shell b lst shell c 2nd shell can hold 1 Which of the following element has complete valence shells a Atomic number is 2 b Atomic number is 9 c Atomic number is 17 d Atomic number is 20 2 Which of the following can ful ls duplet rule Refers to the Periodic Table a Ca b Ar c Fe d He 2 Which of the following can ful ls octet rule Refers to the Periodic Table a Si b Ne c l d Ag Periodic Table 0 A method where atoms of elements are arranged based on the atomic numberproton number Useful in Identify the relative atomic mass and atomic number Identify the chemical symbol and name of the element Determine an element39s properties by understanding the trends present Practice Questions 3 1 What are the functions of the Periodic Table It is useful in which area 2 How many Groups and Periods in the Periodic Table 3 The arrangement of the elements in the Periodic Table are according to their a Bond types b Similar properties c Physical structure d None of the options 2 Based on the Periodic Table state a The relative atomic mass of i Carbon ii Magnesium iii Tungsten iv Lead v Arsenic vi Xenon b The atomic number of i Beryllium ii Potassium iii Vanadium iv Copper v Gold vi Nickel b The atomic symbol of i Silver ii Lead iii Mercury iv Iodine v Neon vi Zinc b The Period of i Titanium ii Coba iii Iron iv Manganese v Helium vi Francium b The Group of I Barium ii Polonium iii Argon iv Lithium v Silicon vi Calcium 2 An unknown element has a proton number of 13 and an atom of this element has 14 neutrons What is the number of electrons in an atom of this unknown element 3 If an atom has 9 protons and an atomic mass of 27 it must have 9 electrons and 9 neutrons a True b False 2 Most atoms rarely exist on their own except a Oxygen b Hydrogen c Water d Noble gas Types of Bonding Formation of chemical bonds Transfer of electrons ionic bonds 0 Sharing of electrons covalent bonds Practice Questions 4 1 Give a function for the atoms involved in the bonding 2 What are the similarity and difference of the ionic bond and covalent bond 3 Determine the type of bonding the atoms go through a F2 b LiF C CO2 d KCI e NH3 2 State the type of bonding and resulting chemical formula when the following atoms are combined a Na and O b H and Cl C O and 0 d AI and O 2 Which of the following shows the correct chemical formula for the compound formed between Carbon and Sulphur a C52 b C25 c CS d C253 2 Determine what are the charges of the following ions after losing or gaining electrons a Na b O c CI d Mg e AI 2 Magnesium undergoes covalent bonding with chlorine to form a compound a True b False 2 Which of the following shows the correct number of protons neutrons and electrons for a sodium atom Na Protons Neutron Electron 5 s a 11 11 12 a 11 12 11 a 11 23 12 a 23 23 11 1 Which of the following shows the correct number of protons neutrons and electrons for a sodium ion Naf Protons Neutron Electron 5 s a 10 12 10 Atomic Radius ls measured by the distance between its nucleus and its valence electron Nuclear charge refers to the total charge of the protons and it measures the attractive forces between the nucleus and the electrons For the atoms with electrons occupying more than one electron shell the inner electrons tend to repel the valence electrons ie shielding effect 0 Due to the increasing attractive force from the nucleus the atomic radii of atoms decrease across the Period 0 Due to the increase in number of electron shells the atomic radii of atoms increase down the Group Practice Questions 5 1 Based on what you learnt so far propose the various Periodic Table trends in the table below Periodic Table lncreaseDecreaseUncha trend nged Across the Period Number of protons Number of electrons Atomic radius Down the Group Number of protons Number of electrons Atomic radius 1 The atomic radius of an atom is indicated by the distance of the valence electrons from the nucleus a If an atom has a higher nuclear charge will the valence electrons be closer to or further from the nucleus Explain your answer b If an atom has a lower nuclear charge will the valence electrons be closer to or further from the nucleus Explain your answer c If an atom has more electrons in the inner shells will the valence electrons be closer to or further from the nucleus Explain your answer d If an atom has less electrons in the inner shells will the valence electrons be closer to or further from the nucleus Explain your answer 2 It is found out that across the period atomic radius decreases a Comparing Atoms Be and B which effect nuclear charge or shielding effect is more signi cant in determining atomic radius across the penod b Explain your answer 2 It is found out that down the group atomic radius increases a Comparing Atoms Be and Mg which effect nuclear charge or shielding effect is more signi cant in determining atomic radius down the group b Explain your answer 2 Discuss and explain the difference in the radius of a An atom of chlorine Cl and its corresponding ion Cl39 b An atom of sodium Na and its corresponding ion Na 2 For the two sets of atoms below Set 1 Na AI S Set2 Br F Cl identify the atom with the a Largest atomic radius b Smallest atomic radius Learning Outcomes 1 An atom is composed of protons and neutrons found inside the nucleus with electrons revolving around this nucleus 2 Most atoms attain stability by forming chemical bonds which takes place either through the transfer of electrons or sharing of electrons 3 The atomic radius of an atom can be in uenced by the nuclear charge and the number of inner electrons present Need answers Feel free to drop me an email 15043445 myrpedusg