Answer: The rows of the periodic table represent the highest energy level of that element.
The columns represent how many valence electrons that element has.
Groups are the same thing as columns, they represent how many valence electrons am element has.
The blocks of the periodic table represent what sublevel(s) the valence electrons fill.
Explanation: Yes
Answer:
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Explanation:
Blocks
Atomic symbol is the one- or two-letter symbol for each element.
Atomic number is the number of protons in the nucleus, which determines the order of elements on the periodic table. This is also the total number of electrons in neutral atoms of the element.
Atomic mass is the mass in grams of 1 mole of atoms. Note that 1 mole contains 6.022·1023 atoms.
Groups
The first two groups of the periodic table(Alkali metals and Alkali Earth metals) are the s-block. Note that helium, in the last column of the table, is also part of the s-block. The outermost electrons of these elements are in s orbitals.
The transition metals make up the d-block, with electrons filling d orbitals. The lanthanides and actinides make up the f-block, with electrons filling f orbitals.
Groups 13 through 18,(post transition metals, metalloids, Reactive nonmetals, and Noble gases-)except for helium, make up the p-block. The outermost electrons of these elements are in p orbitals.
Sections
Metals are more likely to lose valence electrons
nonmetals are more likely to accept electrons.
Metalloids may act like metals or nonmetals, either losing or gaining valence electrons depending on the situation.
Transition metals(groups 3-12) behave somewhat differently because they can lose electrons from their outermost s or d orbitals.
Noble gases are the elements in group 18 that don’t tend to react with other elements. Noble gases have completely filled outer electron shells, as you can see because they’re at the end of each period. The electrons in these elements are stable, making the elements unreactive.
Periods and Groups
Groups of elements have similar properties in terms of how they react with other elements.
All elements in a row have the same number of electron shells. Each next element in a period has one more proton and is less metallic than its predecessor.
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