Plus, what are examples of chemical property trends of the periodic table?
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the short answer is valence shell electrons.
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Alkali earths are the elements of group 2.\nAlkali metals are the elements of group 1.\n\nHere are the properties of group 2\nhttp://en.wikipedia.org/wiki/Alkaline_earth_metal\n\nHere are the properties of group 1\nhttp://en.wikipedia.org/wiki/Alkali_metal\n\nYou can compare them.\n\nHere is the water reaction with elements of group 1 (example K)\n\n2K (s) + 2H2O (l) → 2KOH (aq) + H2 (g)\n\nHere is the water reaction with elements of group 2 (example Mg)\n\nMg + 2H2O → Mg(OH)2 + H2\n\nAs you go to the extremes of the table and down the table the reactivity is higher because the electronegativiy is lower so they have a greater tendency to lose the electron and react.
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Transition metal.\n\nName: Copper \nSymbol: Cu \nAtomic Number: 29 \nAtomic Mass: 63.546 amu \nMelting Point: 1083.0 °C (1356.15 K, 1981.4 °F) \nBoiling Point: 2567.0 °C (2840.15 K, 4652.6 °F) \nNumber of Protons/Electrons: 29 \nNumber of Neutrons: 35 \nClassification: Transition Metal \nCrystal Structure: Cubic \nDensity @ 293 K: 8.96 g/cm3 \nColor: red/orange
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Ionization energy (1st ionization) increase as you go up and right on the periodic table, so fluorine has the highest.  Similar trends are noted in electronegativity.  Fluorine is the element with the highest electronegativity.\n\nThis trend in electronegativity is seen because going down the group you see the successive atoms have more electron levels which puts the valence electrons farther from the nucleus and easier to remove.  Going to the left on the table you are not adding any more electron levels, but the nuclei are becoming increasingly larger and therefore creating a stronger attraction for the valence electrons.
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Copper is #29 on the period table (yes, 4th period), but notice it's average atomic mass is 63.55.  Since electrons weight practically nothing, that means the weight of the protons and neutrons is 63.55.  Since it is #29, it has 29 protons by definition.  So on average it has 63.55 - 29 = 34.55 neutrons.\n\nRemember that though an element has roughly the same number of neutrons as protons, each atom can have a different number of neutrons.  These are called "isotopes".  But on average, copper has 34.55, according to the periodic table I've cited below.
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The Periodic Table of Elements organizes all the elements known to man. There are certain characteristics of each elements that they are grouped by. For example, the last column on the right is called the "Noble Gasses" becase they are all gasses in their natural state, and they're atoms have every electron in each orbital making them the most stable elements.
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Oxidation numbers: tell which atoms lose or gain electrons in chemical reactions, they can be determined by electronegativity\n\nThis web-site lays it out for you and gives examples.\n\nhttp://st19.startlogic.com/~honorsph/honorsphysicalscience/chemical%20formulas/writing_formulas.htm
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I would think your teacher is asking you about the way elements are grouped in the periodic table. You'll notice, for example, that gases are grouped together.\n\n Do a google on "classification of elements" -- there is a lot of stuff out there, and I'm sure it's also in your science text.
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→ Atomic radius decreases → Ionization energy increases → Electronegativity increases →\n\nIn general, the degree of electronegativity decreases down each group and increases across the periods, as shown below. Across a period, non-metals tend to gain electrons and metals tend to lose them due to the atom striving to achieve a stable octet. Down a group, the nuclear charge has less effect on the outermost shells. Therefore, the most electronegative atoms can be found in the upper, right hand side of the periodic table, and the least electronegative elements can be found at the bottom left. \n\nGenerally speaking, atomic ionization energies decrease down a group of the periodic table, and increase left-to-right across a period. Ionization energy exhibits a strong negative correlation with atomic radius.
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You should try the "Physics Handbook", the "Handbook of Thin Film Technology"\n\nThe Handbook of Physicochemical Properties of the Elements (but this one may be available only in russian).\n\nYou may also try this article in an university library:\n\nL. Vitos, A. V. Ruban, H. L. Skriver, and J. Kollar, The surface energy of metals, Surf. Sci. 411, 186 (1998).
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1. NaCN\n2. NO2\n3. CuCl2\n4. NaC2H3O2 \n5. F2\n6. bonding involves transfer of electrons between atoms
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1) Zinc Chloride\n2) Copper (II) Sulphate\n3) there is no such thing as NH4OH, but oh well..\n    Ammonium Hydroxide\n4) Iron (III) Sulphide\n5) Aluminium Phosphate\n6) Lead (II) Nitrate\n7) Sulphur hexafluoride\n8) Sodium Sulphate\n9) Mercury (II) oxide\n10) Potassium Clorate (V)\n11) Tin (II) Choride\n12) Iron (II) hydroxide\n13) Mercury (II) Sulphate\n14) Carbon Dioxide
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There are a few ways to approach this problem.\n\nFirst, on the left side of the periodic table, most elements are cationic in nature--that is, they like to form a positively charged ion. Elements on the right side of the periodic table tend to be anionic, or negavitely charged.\n\nSecondly, elements on the left side of the periodic table are predominantly metals. Those on the right side of the periodic table are mainly non-metals.\n\nAnother significant difference between the left and right sides of the periodic table is the atomic radii of the elements. Elements to the right side of the periodic table are larger in radius than the elements to the left side of the periodic table.\n\nFinally, elements on the right side of the periodic table are usually (although not always) more electronegative than those found on the left side of the periodic table.\n\nI hope this is enough information to help you with your problem. Good luck!
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http://www.chemguide.co.uk/atoms/bonding/vdw.html
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Titanium is a chemical element in the periodic table that has the symbol Ti and atomic number 22. It is a light, strong, lustrous, corrosion-resistant (including resistance to sea water and chlorine) transition metal with a white-silvery-metallic colour. Titanium is used in strong light-weight alloys (most notably with iron and aluminium) and its most common compound, titanium dioxide, is used in white pigments. Examples in which white pigment, consisting of titanium oxide, is used, are correction fluid and commonly used white paint to repaint walls. It is also used in toothpaste, white road marking paints and in white fireworks. Substances containing titanium are called titaniferous.\n\nThe element occurs in numerous minerals with the main sources being rutile and ilmenite, which are widely distributed over the Earth. There are two allotropic forms and five naturally occurring isotopes of this element; 46Ti through 50Ti with 48Ti being the most abundant (73.8%). One of titanium's most notable characteristics is that it is as strong as steel but is only 60% its density. Titanium's properties are chemically and physically similar to zirconium.\nContents\n[hide]\n\n    * 1 Notable characteristics\n    * 2 Applications\n    * 3 History\n    * 4 Occurrence\n    * 5 Isolation\n    * 6 Compounds\n    * 7 Isotopes\n    * 8 Precautions\n    * 9 See also\n    * 10 References\n    * 11 External links\n\n[edit]\n\nNotable characteristics\n\nTitanium is well known for its excellent resistance to corrosion; it is almost as resistant as platinum, being able to withstand attack by acids, moist chlorine gas, and by common salt solutions. Pure titanium is not soluble in water but is soluble in concentrated acids. A metallic element, it is also well-known for its high strength-to-weight ratio. It is a light, strong metal with low density that, when pure, is quite ductile (especially in an oxygen-free environment), easy to work, lustrous, and metallic-white in colour. The relatively high melting point of this element makes it useful as a refractory metal. Commercially pure grades of titanium have an ultimate tensile strength equal to that of intermediate strength high strength low alloy steels, but are 43% lighter; it is 60% heavier than aluminium, but more than twice as strong as 6061-T6 aluminium alloy; these numbers can vary quite substantially due to different alloy compositions and processing variables. They are included as guidelines only.\n\nThis metal forms a passive and protective oxide coating (leading to corrosion-resistance) when exposed to elevated temperatures in air but at room temperatures it resists tarnishing. The metal, which burns when heated in air 610 °C or higher (forming titanium dioxide) is also one of the few elements that burns in pure nitrogen gas (it burns at 800 °C and forms titanium nitride). Titanium is resistant to dilute sulfuric and hydrochloric acid, along with chlorine gas, chloride solutions, and most organic acids. It is paramagnetic (weakly attracted to magnets) and has a very low electrical resistivity and thermal conductivity.\n\nExperiments have shown that natural titanium becomes very radioactive after it is bombarded with deuterons, emitting mainly positrons and hard gamma rays. The metal is a dimorphic allotrope with the hexagonal alpha form changing into the cubic beta form very slowly at around 880 °C. When it is red hot the metal combines with oxygen, and when it reaches 550 °C it combines with chlorine. It also reacts with the other halogens and absorbs hydrogen.\n[edit]\n\nApplications\nwatch with titanium cover\nEnlarge\nwatch with titanium cover\n\nAbout 95% of titanium production is consumed in the form of titanium dioxide (TiO2), an intensely white permanent pigment with good covering power in paints, paper, toothpaste, and plastics. Paints made with titanium dioxide are excellent reflectors of infrared radiation and are therefore used extensively by astronomers and in exterior p
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hydrogen is the entity we find everywhere.coming to its ionic properties it loses the one electron it has and forms H+ ion.this property gives the acidic property.\nwhen it is losing an electron it is getting oxidised and  when any other atom takes that electron it is reduced.\nfor example: H2 +F2 gives 2HF.\nin this hydrogen gives off its electron to flourine and gets oxidised and reduces the flourine by giving its electrons.
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Mendeleev, a Russian Chemist, was one of the first to be partially sucessful in arranging the known elements in the 1870's into a chart that would allow the prediction of properties. He arranged the elements known in those days according to increasing atomic masses. The first Periodic Law proposed by him stated:\n\n"The properties of the elements are a periodic function of their atomic masses"\n\nWhen Mendeleev arranged the known elements using this principle as a guide, he found that certain elements grouped themselves into vertical groupings sometimes called families. If one measured a property of each of the elements in the group, Mendeleev noted that the value for that property would either be high or low depending upon the group under observation. For example, measuring the atomic radius of the atoms of elements which is the distance from the outermost valence region to the nucleus of an atom, one would find that in the case of the first group of elements on the left side of the chart all the elements seemed to have characteristically high values where those elements grouped on the right side of the chart seemed to have characteristically small radii values. All of the elements in group 1 had the highest radius value of any element in its respective period. A period is a horizontal row of elements in the table. Likewise all the elements in group 17 on the far right of the chart had the lowest radius value of any element in its respective period. This is a manifestation of the periodicity exhibited by the elements between their atomic weights and their property measurements. One could conceivably show this periodicity using other properties such as boiling points, melting points, etc.