elements, ions, & isotopes\nname ayami atanis\nread\nelements are pure substances made up of only one type…

elements, ions, & isotopes\nname ayami atanis\nread\nelements are pure substances made up of only one type of atom, like gold, oxygen, or hydrogen. each atom has a center called a nucleus, which holds two types of tiny particles: protons and neutrons. the number of protons in an atom decides what element it is. surrounding the nucleus are even smaller particles called electrons that move around quickly.\nions form when atoms gain or lose electrons. valence electrons: the electrons in the outermost shell of the atom, which gives them an electric charge. if an atom gains electrons, it becomes a negative ion. if it loses electrons, it becomes a positive ion. isotopes are different versions of the same element. they have the same number of protons but a different number of neutrons, so they weigh a bit more or less. even though theyre heavier or lighter, isotopes still have the same chemical properties because theyre still the same element.\ndefine the following terms:\nelement \nisotope \nion different versions of the same element.\nexcited state \nvalence electrons \ncarbon 12\n6 protons\n6 neutrons\ncarbon 13\n6 protons\n7 neutrons\ncarbon 14\n6 protons\n8 neutrons\n1. what is the difference between carbon - 12, carbon - 13, and carbon - 14?\n2. why do differing numbers of neutrons not change the overall electric charge of an element, or the element itself?\n47.867\n+2\n+3\n+4\nti\n22\n2 - 8 - 10 - 2\non the element above, use arrows to label: chemical symbol, atomic number, atomic mass, oxidation states, electron configuration.\ncircle the ions below. remember ions have a positive or negative charge\nca²⁺ n₂ h₂o k⁺ no₃⁻ nacl

elements, ions, & isotopes\nname ayami atanis\nread\nelements are pure substances made up of only one type of atom, like gold, oxygen, or hydrogen. each atom has a center called a nucleus, which holds two types of tiny particles: protons and neutrons. the number of protons in an atom decides what element it is. surrounding the nucleus are even smaller particles called electrons that move around quickly.\nions form when atoms gain or lose electrons. valence electrons: the electrons in the outermost shell of the atom, which gives them an electric charge. if an atom gains electrons, it becomes a negative ion. if it loses electrons, it becomes a positive ion. isotopes are different versions of the same element. they have the same number of protons but a different number of neutrons, so they weigh a bit more or less. even though theyre heavier or lighter, isotopes still have the same chemical properties because theyre still the same element.\ndefine the following terms:\nelement \nisotope \nion different versions of the same element.\nexcited state \nvalence electrons \ncarbon 12\n6 protons\n6 neutrons\ncarbon 13\n6 protons\n7 neutrons\ncarbon 14\n6 protons\n8 neutrons\n1. what is the difference between carbon - 12, carbon - 13, and carbon - 14?\n2. why do differing numbers of neutrons not change the overall electric charge of an element, or the element itself?\n47.867\n+2\n+3\n+4\nti\n22\n2 - 8 - 10 - 2\non the element above, use arrows to label: chemical symbol, atomic number, atomic mass, oxidation states, electron configuration.\ncircle the ions below. remember ions have a positive or negative charge\nca²⁺ n₂ h₂o k⁺ no₃⁻ nacl

Answer

Brief Explanations:

  1. For the first question, we look at the number of neutrons in each isotope. Carbon - 12 has 6 neutrons, Carbon - 13 has 7 neutrons, and Carbon - 14 has 8 neutrons. The difference between Carbon - 13 and Carbon - 12 is 1 neutron (7 - 6 = 1), and between Carbon - 13 and Carbon - 14 is 1 neutron (8 - 7 = 1). For the second question, neutrons are neutral particles, so changing their number does not affect the overall electric charge which is determined by protons (positive) and electrons (negative). Also, the element is defined by the number of protons, not neutrons. For the definitions:
  • Element: A pure substance made of only one type of atom.
  • Isotope: Different versions of the same element with the same number of protons but different number of neutrons.
  • Ion: An atom that has gained or lost electrons, resulting in a positive or negative charge.
  • Excited State: A state of an atom where electrons are in higher - energy orbitals than the ground state.
  • Valence Electrons: The electrons in the outermost shell of an atom. For the element Ti:
  • Chemical symbol: Ti
  • Atomic number: 22
  • Atomic mass: 47.867
  • Oxidation states: +2, +3, +4
  • Electron configuration: 2 - 8 - 10 - 2 The ions are $Ca^{2 +}$, $K^{+}$, $NO_{3}^{-}$.

Answer:

  1. The difference between Carbon - 13 and Carbon - 12, and Carbon - 13 and Carbon - 14 is 1 neutron each. Neutrons are neutral, so changing their number does not change the electric charge and the element is defined by the number of protons.
  2. Element: A pure substance made of only one type of atom. Isotope: Different versions of the same element with the same number of protons but different number of neutrons. Ion: An atom that has gained or lost electrons, resulting in a positive or negative charge. Excited State: A state of an atom where electrons are in higher - energy orbitals than the ground state. Valence Electrons: The electrons in the outermost shell of an atom. For Ti: Chemical symbol is Ti, atomic number is 22, atomic mass is 47.867, oxidation states are +2, +3, +4, electron configuration is 2 - 8 - 10 - 2. Ions are $Ca^{2 +}$, $K^{+}$, $NO_{3}^{-}$