physci - quiz 1 reviewer.pdf

PHYSCI WA1 Juana Gabriella N. Gozum | 11ABM-13 Module 1: Origin and Formation of Elements in the Universe Bing Bang Theory ➔ the most accepted and endorsed theory of the origin of the universe ➔ it all started from the two Nucleosynthesis...

PHYSCI WA1 Juana Gabriella N. Gozum | 11ABM-13 Module 1: Origin and Formation of Elements in the Universe Bing Bang Theory ➔ the most accepted and endorsed theory of the origin of the universe ➔ it all started from the two Nucleosynthesis observations of Edwin Hubble: Nucleo = Nucleus 1. The Milky Way is not the only Synthesis = Formation existing galaxy. 2. The galaxies are in constant The nucleus is made up of protons and motion, moving away from neutrons. Before their formation, protons each other. and neutrons were called quarks and ➔ The birth of the theory was made gluons. by Georges Lemaitre, who asked, “How did the universe start?” Nucleosynthesis and Primordial Elements ➔ Once the deuterium bottleneck was cleared in the early universe, the newly formed deuterium could undergo further nuclear reactions to form higher elements. ➔ Nuclear fusion: a nucleus combines with another nucleus to form larger nuclei ➔ Nuclear fission: a nucleus splits into smaller nuclei Cosmic Origin of Elements Big Bang Nucleosynthesis (Big Bang and Cosmic Ray Nucleosynthesis) Hydrogen (H), Helium (He), and trace amounts of Lithium (Li) PHYSCI WA1 Juana Gabriella N. Gozum | 11ABM-13 Stellar Nucleosynthesis (Small and Large Stars Nucleosynthesis) From Beryllium (Be) to Iron (Fe) Supernova Nucleosynthesis (Stellar Explosion) From Cobalt (Co) to Uranium (U) Atoms, Ions, and Isotopes What is an Ion? - an ion is an atom or molecule with a net electric charge PHYSCI WA1 Juana Gabriella N. Gozum | 11ABM-13 Module 2: Trends in the Periodic Table of Elements Alkali Metals - their reaction with water forms alkalies. strong bases that can neutralize acids Alkaline Earth Metals - these reactive metals form divalent cations and are malleable and ductile. Transition Metals - these elements can form stable cations with an incomplete filled d orbital. Post-transition metals - also known as poor metals. they are to the right of the transition metals Metalloids - have properties intermediate between those of metals and non-metals Nonmetals - do not produce heat or electricity and are structurally brittle Halogens - nonmetals that consist of diatomic molecules. when they react with metals, they produce ionic compounds (salts) Noble gases - are referred to as the “inert gases” since their filled valence shells (octets) make them nonreactive to other elements. Atomic Radius - the total distance from an atom’s nucleus to the outermost orbital of an electron; used to measure the size of an atom Electron Affinity - the amount of energy released when an electron is added to a neutral atom to form an anion, an atom PHYSCI WA1 Juana Gabriella N. Gozum | 11ABM-13 with high affinity more easily accepts Module 3: Chemical Bonds, LEDS, and electrons Electronegativity Electronegativity - the tendency of an atom participating in a covalent bond to Lewis Electron Dot Structure (LEDS) attract the bonding electrons; the higher ➔ Gilbert Newton Lewis the electronegativity, the more strongly ➔ Representation of the valence that element attracts the shared electrons electrons of an atom that uses dots Ionization energy - the quantity of energy around the symbol of an element that an isolated, gaseous atom in the For transition metals: ground electronic state must absorb to ➔ Unlike main group elements, discharge an electron, resulting in a cation; transition metals typically do not higher ionization energy shows a high use Lewis dot structures. attraction between the electron and the ➔ Variable valence nucleus. ➔ Involvement of d-orbital Metallic Character - the tendency of an element to lose electrons and form (+) ions (cations) Nonmetallic Character - the tendency of an element to accept electrons and form (-) ions (anions) Chemical Bonds Elements ➔ Constitute the simplest chemical substances in which all the atoms are the same. ➔ Examples: He, Fe, C, K ➔ Elemental molecules: H2, N2, F2, O2, I2, Cl2, Br2 PHYSCI WA1 Juana Gabriella N. Gozum | 11ABM-13 Compounds Notable Scientists ➔ Chemical substances are made up Robert Boyle - elements and atomism of two or more elements that are Joseph Priestley - combustion; phlogiston chemically bound together in a theory fixed ratio. Joseph Proust - law of definite proportion ➔ Question: What is the difference John Dalton - law of multiple proportions between compounds and Anton Lavoisier - law of conservation of molecules? mass Mixture ➔ Combination of compounds, Chemical Bonds elements, and altogether in one ➔ Results from the transfer of one or chemical substance. more valence electrons from one atom to another. ➔ Exists between a metal (M) that tends to lose electrons and a nonmetal (NM) that tends to accept electrons. ➔ Two types of ions participate in ionic bonding: monoatomic and polyatomic ions. Chemical Bonds ➔ Refers to the formation of a chemical bond between two or more atoms, molecules, or ions to give rise to a chemical compound. Monoatomic Ions PHYSCI WA1 Juana Gabriella N. Gozum | 11ABM-13 ➔ An ion made of exactly one atom Transition metals in ionic bonding. Write the ➔ An atom that has an unequal number chemical formula of the following: of protons and electrons 1. Iron (II) and sulfate ➔ Depending on the charge, these ions 2. Cobalt (II) and nitrogen may be classified as cations or anions. 3. Lead (IV) and chlorine Ionic Charfes of Elements (as monoatomic Lewis Electron Dot Structure (LEDS) of ionic ions) compounds: 1. At the start of the crisscross method, Polyatomic Ions the number of electrons to be donated ➔ If the compound is made up of two or by the cation (metal) and accepted by more atoms, it can be referred to as a the anion (nonmetal) is indicated as polyatomic ion or a molecular ion. superscripts. This will represent the ➔ Depending on the charge, these ions charges of the elements. may also be classified as cations or 2. At the end of the crisscross method, the anions. subscripts will be the coefficient of the elements. Writing the chemical formula 3. The metal (cation) should have no 1. Write the chemical symbol of the Lewis dots since it donated all its elements. valence eletron/s; while the nonmetal 2. Write the number of electrons to be (anion) should be drawn with eight donated or accepted by each element. Lewis dots sine it gained additional 3. Criss-cross the number of electrons valence electron/s. and drop as subscripts. 4. The element symbols and their LEDS 4. Simplify the numbers if necessary (for must be placed inside a bracket, and the same numbers, even numbers) the corresponding charges and coefficients are placed outside. Monoatomic ions in ionic compounds. Write the chemical formula of the following: Lewis Electron Dot Structure (LEDS) of ionic 1. Sodium and oxygen compounds 2. Magnesium and bromine Examples: Monoatomic ions and transition 3. Beryllium and sulfur metal ions 1. Sodium and chlorine Polyatomic ions in ionic bonding. 2. Iron (II) and bromine Write the chemical formula of the following: 1. Sodium and hydroxide Lewis Electron Dot Structure (LEDS) of ionic 2. Magnesium and phosphate compounds 3. Calcium and sulfate Examples: Polyatomic Ions 1. Calcium and hydroxide ion 2. Magnesium and sulfate ion PHYSCI WA1 Juana Gabriella N. Gozum | 11ABM-13 Lewis Electron DotStructure (LEDS) of ionic ➔ The number of electrons shared by compounds - Examples: Monoatomic the adjacent atoms will be the ions same. ➔ Occurs in bonding atoms that have similar or identical electronegativities. Covalent Bond ➔ Results from the sharing of one or more valence electrons from one Polar Covalent Bond atom to another. ➔ Formed when electrons are shared ➔ Exists between two nonmetals (NM) unequally between two nonmetals. ➔ Two types: nonpolar and polar ➔ The number of electrons shared will covalent bonds. be the different. ➔ Occurs in bonding atoms that have different electronegativities. ➔ Procedures electrical dipoles (partial charges) between atoms. Nonpolar Covalent Bond ➔ A type of bond that is formed when electrons are shared equally between two nonmetals. PHYSCI WA1 Juana Gabriella N. Gozum | 11ABM-13 PHYSCI WA1 Juana Gabriella N. Gozum | 11ABM-13