Stage 2, Matter and its transformation

Atomic theory known as "Cloud of electrons model". Thomson. Dalton. Shrödinger. Rutherford.

He presented a particle that found in the nucleus of the atom, that have not charge and he called neutron. Thomson. Dalton. Chadwick. Rutherford.

Model that present a nucleous in the center of an atom. Thomson. Dalton. Chadwick. Rutherford.

Correspond to the numbers of protons that are in the nucleus of the atom and is the responsible of nuclear positive charge. Atomic number. Oxidation number. Mass number. Nucleus number.

They are atoms with same charge, have the same atomic number but different mass number. Electrons. Neutrons. Protons. Isotopes.

Name of the circular orbitals accordance with Bohr model. Electronic cloud. Orbitals. Energy levels. Unit of atomic mass.

Is the sum of protons and neutrons. Atomic number. Molecula weight. Mass number. Atomic weight.

Analyze the following isotope and calculate the number of protons, neutrons and electrons Ca A=40 Z=20. p= 40 e=20 n=40. p= 20 e=20 n=20. p= 20 e=20 n=40. p= 20 e=20 n=60.

Region around the nucleus where can found, with higher probability, one electron in the atom. Orbits. Atomic orbital. Nucleus. Atomic quantum.

Model that preserve the basic principles of atomic model of Bohr; the orbits they become in orbitals, and the electron can not found in a specific place, without it existing the probability located it in a specific region called atomic orbital. Atomic model of Dalton. Atomic model of Rutherford. Atomic model of Thomson. Quantum atomic model.

Is the form of write how are accommodated the electrons of every atom in their orbitals. Aufbau principle and diagonal rule. Pauli exclusion principle. Electronic configuration. Hund rule.

Establishes that in an atom can not existing two electrons that can have their four quantum numbers equals. Aufbau principle and diagonal rule. Pauli exclusion principle. Electronic configuration. Hund rule.

Rule that indiques how make it filling of the electrons in the orbitals, depending of their energy. Aufbau principle and diagonal rule. Pauli exclusion principle. Electronic configuration. Hund rule.

Select the option that correspond to the electronic configuration of 6C. 1s2, 2s2, 2p2. 1s2, 2p2, 2s2. 1s2, 1p2, 2s2. 1s2, 2p2, 2d2.

Select the option that correspond to the electronic configuration of 20Ca. 1s2, 2s2, 2p6, 3s2, 3p6, 4s2. 1s2, 2s2, 3p6, 3s2, 3p6, 4s2. 1s2, 2s2, 3p6, 4s2, 3p6, 4s2. 1s2, 2s2, 3p6, 4s2, 5p6, 6s2.

In the experimental practice "Flame test", some metals were identified, heating a sample in the flame. According with the results, relates every metal describe in the left column with the flame´s color 1. Lithium 2. Sodium 3. Copper a. Green b. Golden c. Yellow d. Red. 1d, 2b, 3c. 1d, 2a, 3b. 1d, 2c, 3a. 1c, 2b, 3c.

Correspond to the numbers of protons that are in the nucleus of the atom and is the responsible of nuclear positive charge. Oxidation number. Atomic number. Mass number. Weight.

Proposed hypotheses on the nature of matter and thus, set the stage for his atomic theory in 1808. John Dalton. J.J Thomson. Bohr. Rutherford.

Used the tube of cathode rays, identified that this rays are affected by electric camp and that attracted by a positive part, so it was concluded that they were composed of negative particles called electrons. John Dalton. J.J Thomson. Bohr. Rutherford.

Suggested the first model of the atom, considering it as a compact, homogeneous, indivisible sphere with a positive charge in which the electrons were embedded as if they were raisins in a pudding. John Dalton. J.J Thomson. Bohr. Rutherford.

He also concluded that if the atom had electrons in order to neutralize the negative charge, positively charge in the same amount with high concentration, which he called the atomic nucleus. John Dalton. J.J Thomson. Bohr. Rutherford.

Proposed a model when: Atoms have only certain allowable energy states. Electrons moved around the nucleus in only certain allowed circular orbits. John Dalton. J.J Thomson. Bohr. Rutherford.

In the isotopic notation, A represents: Mass number. Atomic number. Chemical symbol. Chemical Formula.

Establishes that, when filling orbitals with the same energy the electrons are distributed, always that its possible, with their parales spins, that is to say, unpaired and occupying the maximun possibles orbitals. Aufbau principle and diagonal rule. Pauli exclusion principle. Electronic configuration. Hund rule.

With what letters are the atomic orbitals designated: s, p, d, f. a, b, c, d. n, l, m, s. s, n, f, z.