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NAME DATE PER EKS 2: Atomic Structure Quiz Study Guide Level 2 Vocabulary Atom: smallest unit of matter. Looks like planetary model, with a dense positively charged nucleus in the middle, and electrons orbiting the outside. Isotope: heavier and lighter versions of the same element. The masses of isotopes differ because they have different amounts of neutrons. Ion: an atom with a net electrical charge. Ions have charges because they gain or lose electrons. Negatively charged ions (anions) gain electrons. Positively charged (cations) ions lose electrons. Proton: positively charged particle located in the nucleus. The number of protons defines the atom and never changes. Neutron: neutral particles located in the nucleus. Electron: negatively charged particles that make up most of an atom’s volume. Atomic Number: small number on the periodic table, number of protons an element has Mass Number: how heavy an atom is, can be calculated by adding P+N Chemical Symbol: 1 or 2 letter abbreviation for an element given on the periodic table Planetary Model: idea that an atom looks like the solar system, with electrons orbiting around the nucleus. (the Rutherford experiment supported this model) Plum Pudding Model: idea that the atom was positively charged, with electrons sprinkled throughout it. The Rutherford experiment suggested that this model was inaccurate. Mass: how heavy something is. An atom’s mass is made up of protons and neutrons’ masses Volume: how much space something takes up. Electrons make up most of an atom’s volume Level 3 Practice Questions 1. A) Write an equation that shows how to figure out how many neutrons an atom has. Neutrons= mass- protons B) Explain why the equation makes sense. This makes sense because protons and neutrons are the heaviest subatomic particles. Mass of protons+ mass of neutrons= mass of nucleus (where an atom gets most of its weight). Electrons are not included in the equation because electrons do not contribute to an atom’s mass. NAME DATE PER 2. Fill in the chart. Chemical Symbol P Na+ Li—8 Protons Neutrons Electrons Atomic # Mass # Net Charge 15 11 3 16 12 5 15 10 3 15 11 3 31 23 8 0 +1 0 Level 4 Practice Questions 1. Rutherford designed an experiment to see whether an atom looked like the solar system or plum pudding. In his experiment, Rutherford shot gold atoms with a positively charged particle beam. Write a hypothesis for what would have happened in the experiment if Rutherford used a negatively charged particle beam instead. (try to follow the 4 hypothesis rules that we learned in class!) If the atom is shot with a negative particle beam, then the beam will deflect from electrons orbiting the outside of the atom. OR If the atom is shot with a negative particle beam, then the beam will attract to the nucleus in the center, and will not exit the atom. 2. Some atoms are more likely to gain electrons and become negatively charged ions. Some atoms are more likely to lose electrons and become positively charged ions. Using what you know about what an atom looks like, explain why you think this is true. (hint: think about the charges of protons and electrons!) Atoms with more protons have a stronger positive charge in their nucleus. This positive charge can attract the negatively charged electrons from other atoms. Atoms with few protons in their nucleus cannot attract electrons as well, and might lose their electrons.