Flashcards
Atomic Structure and Periodicity
Flashcards do conjunto (26)
- 1Draw the model of an Atom.
- 2What is an Atom?An atom is the smallest particle of an element.
- 3What are Isotopes?Different atomic forms of the same element, which have the same number of protons but a different number of neutrons.
- 4What is the Relative Atomic Mass?The Relative Atomic Mass of an atom is the weighted average of the naturally occurring isotopes of an element.
- 5What is the Atomic number and Mass number? How to calculate the number of neutrons in an atom? Explain using an example.
- 6What are Valance Electrons?Valance electrons are electrons in the outermost shell (furthest from the nucleus). They determine the chemical properties. Atoms can lose or gain valence electrons to form charged particle called ions
- 7What are Ions?Ions are formed when an atom loses or gains electrons.
Cation:
When an atom has an overall positive charge. (Lost 1 or more electrons)
Anion:
When an atom has an overall negative charge. (Gained 1 or more electrons)
In a neutral atom, the number of electrons must match the number of protons. - 8Electron configuration of Shells.The number of electrons in each shell is equal to 2n². The lowest shells (those closest to the nucleus) have the lowest energy and are always filled first.
- 9Electron configuration of Sub-shells.
- 10What is the valence electron trends in the periodic table?
- 11What is a period? What is a group?The period is the horizontal row of electrons in the periodic table.
The group is the vertical column of elements in the periodic table. Elements in the same group behave chemically similar. - 12What is the exception in Electronic Configuration?Chromium and copper are exception in which a completely full or half full d sub-level is more stable than a partially filled d sub-level, so an electron from the 4s orbital is excited and rises to a 3d orbital.
- 13What is a Ground state?The ground state is the lowest energy state of a system.
- 14What is an Excited State?The excited stage is any energy state higher than the ground state. It is the atom has a higher potential energy than it has in its ground state. The excited electron does not stay in the excited state permanently, however and eventually falls back to the ground state.
- 15Identify the Alkali metals, Alkaline Earth Metals, Halogens, Nobel gasses, non-metals, transition metals and metalloids.
- 16Write the first 36 elements in the black periodic table.
- 17What is the Atomic radii?Atomic radii is the atomic size of an atom. Atomic radii decreases as you move across the period from left to right. As the Affective nuclear charge increases, the valance electrons are drawn closer to the nucleus, making it smaller.
- 18What is electronegativity?Electronegativity is the tendency for an atom to attract electrons to itself. Electronegativity increases going across a period, and decreases going down a group. Non-metals are highly electronegative while metals have low electronegativity.
Group: the electrons are further away from the nucleus and better shielded from the nuclear charge and therefore not as attracted to the nucleus
Period: when the nuclear charge increases, so will the attraction that the atom has for electrons in its outermost energy level and that means the electronegativity will increase - 19What is Ionisation energy?Ionisation energy is the energy required to remove an electron from an atom. Ionisation energy increases across a period, and decreases down a group.
- 20What is electron affinity?Electron affinity is the amount of energy released when an atom gains an electron to form a negative ion. Electron affinity increases (becomes more negative) across a period and does not change must down a group.
- 21What is shielding?Shielding is the barrier made of inner-shell electrons and it decreases the nucleus' pull on the outer electrons
- 22What is the Affective nuclear charge?It is the pulling in power.
Calculate:
Protons- inner shell electrons - 23How to arrange species according to their radius. A: Cl, Ar, K B:K, Ar, Cl C: Cl, K, Ar D: Ar, Cl, KThe answer is B. K (19) has the highest nuclear charge, followed by Argon (18) and Chlorine (17).
Nuclear change= positive atomic number - 24What is the Ionisation energy of noble gasses?The ionisation energy of noble gasses is larger than the other groups because they are incredibly stable, and a lot of energy would be needed to remove it's electrons.
- 25What do transition metals ave in common with respect to their electron configuration?All the transition metals are located in the d-block, therefore they gradually fill the shells. They are all in the excited level, therefore they have one less electron in the inside shells. However, the last orbital is always fully.
- 26What are the charges of Groups 1, 2, 13, 15, 16 and 17?
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- 11 Chemistry Stage 1 (Atomic Structure and Periodic Trends ) FlashCards sobre Atomic Structure and Periodicity , criado por Roosi P em 30-06-2016.
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- Roosi P
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