## Elements and also the periodic Table

### Atomic properties

atomic mass: counting the variety of neutrons + protons for the atomic mass. We create the atom mass as a superscript in prior of the atom symbol. The most typical isotope of carbon has actually a mass of 12, 12C.You are watching: How many valence electrons does titanium have

**atomic number**: counting the number of protons in the nucleus for the atom number. The number of electrons in a neutral atom is equal to the number of protons in the nucleus, or the atom number. The atomic number of carbon is 6.

**isotopes**These space atoms that the same facet that different in the number of neutrons. Different isotopes have various natural abundance. Because that hydrogen, the isotope 1H has the highest natural abundance. 1H, 2H, 3H

**12C, 13C, 14C**.

### Electrons

Each electron in an atom is defined by a distinct quantum number**n**, rule quantum number, value= 1, 2, 3...

**l**, orbit quantum number, value= 0, 1, 2...(n-1)

**m**, magnetic quantum number, integral values in between -l and l

**s**, spin quantum number, value= -1/2 or 1/2For l= 0, over there is only one kind of orbital (m= 0), the s orbital. Because that l= 1, p, there are 3 kinds of orbitals (m= -1, 0, 1) that we recognize as the px, py, and also pz orbitals. Because that l= 2, there are 5 type of d orbitals (m= -2, -2, 0, 1, 2). Two electrons at most have the right to occupy every orbital v a spin quantum variety of 1/2 or -1/2. The shapes of the most basic s, p, and d orbitals are presented below.

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The orbitals differ in the number of

**nodes**. A nodal plane is a plane where electron thickness is precisely zero. Look in ~ the sine tide at right. Think the this together a 2 dimensional representation of a ns orbital. The component of the line above the base line encloses the mathematically positive part of the electron density function. The curve below the baseline encloses the mathematically an adverse part of the electron density function. This orbital has a nodal plane, a aircraft where the electron thickness is zero, in ~ the nucleus.The 1s orbital has actually 0 radial nodes, 2p orbitals each have actually 1 node, 3d orbitals have actually 2 nodes, etc.When there are 2 electron in an orbital, their spins (1/2, -1/2) cancel. Only when there room unpaired electrons in orbitals does the atom or molecule have actually a network electron spin.

**Oxidation**= lose of one or much more electrons

**Reduction**= get of one or an ext electrons

**Orbital Energies**There is a different ordering of orbit energies for neutral atoms and for those exact same atoms in ion or molecules where there have the right to be a partial fee on the atom.Neutral, diverted atoms1s Ions and compounds1s