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What do all elements group 1 have in common in terms of electrons?
Wiki User
∙ 6y ago
Group A1 of the Periodic Table (Hydrogen, Lithium, Sodium . . . ) is an Alkali Metal and only has one valance electron. If the element were to lose that electron, it forms an ion. Each element violently reacts when combined with water.
Wiki User
∙ 13y ago
Wiki User
∙ 12y agoAll group 1 elements have one electron in their outermost energy level, or valence shell. Their valence shell electron configurations are all ns1. Because of this they have similar physical and chemical properties.
Wiki User
∙ 7y agoSimilar chemical properties.
They all have 1 valence electron. They will form +1 cations. They are highly reactive with water. They are commonly spectator ions in reactions.
Wiki User
∙ 14y agoThey are all alkiline metals and are all very reactive in water
Wiki User
∙ 13y ago1 electron in the outer shell
low first ionization energy
high second ionization energy
large difference between first and second ionization energy.
Wiki User
∙ 6y agoAll these elements have only one valence electron.
Wiki User
∙ 11y agoThey all have one valence electron.
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In terms of periodic law which of these elements are the most similar - sodium phosphorus and sulfur?
The elements phosphorus and sulfur are elements 15 and 16 on the periodic table. They will have more in common than sodium, element 11 and an Alkali metal from Group 1 of the table, will have with either phosphorus or sulfur.
Calcium and Sodium have very nearly the same radii?
No sodium has 11 electrons which means its valence are in the 3s2 orbit while Calcium has 20 electrons its valence electrons are in the 4s2 orbit which is much larger in terms of atomic radii
What makes an element more massive?
The more protons and neutrons that are in the element and isotope electrons are negligible in terms of mass.
What is terms might be a chemical compound?
A compound contain two or more elements associated by chemical bonds.
What are the four elements of a deductive structure?
Undefined terms; assumptions (postulates); definitions; theorems and other conclusions
Is group 8 the same as group 0?
Both terms are acceptable due to the fact that eight electrons exist in the outermost shell of all elements in the group. Therefore, one could say that this group has 8 electrons in the outermost shell or that there are no electrons in the outermost shell - as the structure is stable! It is the perspective of a person.
In terms of electrons in the periodic table why are group 1 metals very reactive and group 7 non-metals very reactive too?
Atomic elements typically want to have full electron shells ("valence shells"), instead of shells with uneven numbers. Group 1 metals have only 1 electron in their valence shell, so they quickly react to lose this electron and have an empty shell (but a full shell underneath it). Group 7 elements have 7 valence electrons and react quickly to steal another atom's electron and gain a full shell of 8 electrons. This willingness to lose or steal electrons makes the elements very reactive, but in different ways. Group 1 elements will become positively charged ions, and Group 7 will become negatively charged. (Na+ versus Cl-) Group 6 elements (such as oxygen) are also somewhat reactive and will steal 2 electrons to become even more negatively charged (O 2-)
Is the periodic table is most easily understood in terms of the electron configurations of the elements?
Yes. In terms of electron configuration and the number of valence electrons.
Trends in the properties of elements in a group or period can be explained in terms of?
Electron Configuration
What makes elements similar?
By elements being similar, I assume you mean elements of the same group being similar rather than all elements in general. Elements of the same group are similar in terms of chemical properties because they share a similar electron configuration. For instance group one of the periodic table, the alkali metals, has only one electron in its outermost unfilled orbital. Because chemical reactions are dependent on the exchange and sharing of electrons, the similarity of electron configuration in elements of a group results in them having similar properties. For instance, the alkali metals are all soft and extremely reactive.
In terms of periodic law which of these elements are the most similar - sodium phosphorus and sulfur?
The elements phosphorus and sulfur are elements 15 and 16 on the periodic table. They will have more in common than sodium, element 11 and an Alkali metal from Group 1 of the table, will have with either phosphorus or sulfur.
What terms refer to elements in a column of the periodic table?
They are groups
How are all of the nonmetal elements on the periodic table related terms of ability to lose electrons?
All non-metals have either 5, 6 or 7 electrons in their octet which makes them suitable to gain electrons to achieve stability. Hence it is difficult for electrons to lose electrons.
How are all of the non metals elements on the periodic table related in terms of ability to loose electrons?
Nonmetals are closer to a full outer shell. They would rather gain electrons to complete the shell. They are unlikely to lose electrons.
In group 1 in the periodic table which element is most active?
In terms of reactivity, Potassium(K) is the most reactive element among group 1 elements.
What outermost electrons in an atom with the inner electrons of an atom in terms of energy.?
valence electrons
How are oxidation numbers predictable using the periodic table?
In very simple terms to achieve the octet atoms either lose valence electrons or gain them. The number of valence electrons for the period 2 elements is relativelly straightforward use the group number and remember to take 10 away from B, C, N, O and F. So as an example boron in group 13 has 3 valence electrons- so gain of +5 or loss of 3. Gaining five seems so excessive so your best guess is +3, which is true in say B2O3As for using the periodic table to predict- not so easy- take gallium - in group 13 has 3 valence electrons- so it could lose 3 to give an octet, which indeed is its most common ON but can also lose 1 electron to form Ga+
