0
Is this statement true or false Most transition metals lose one electron to form a plus 1 cation.?
Wiki User
∙ 7y agoWant this question answered?
Be notified when an answer is posted
Add your answer:
Earn +20 pts
Is a cation isoelectric with the element before or after it?
No necessarily. Although the alkali metal cations are, most other cation-forming elements (metals) are not as many of them lose more than one electron. It is even more complicate for the transition metals as they can move electrons between their s and d orbitals.
Why are alkali metals more reactive than transition metals?
Groups 3-12 do not have individual names. Instead, all of these groups are called transition metals. The atoms of transition metals do not give away their electrons as easily as atoms of the Group 1 and Group 2 metals do. So, transition metals are less reactive than alkali metals and alkaline-earth metals are.
How does the electron configuration contributes to transition metals?
color, magnetism, conductivity to name a few.
How do the electron configurations of the transition metals differ from those of the metals in groups 1 and 2?
The elements in groups 1A and 2A have valence electrons in s-orbitals, while the elements in groups 3A-8A have valence electrons in p-orbitals.
Are transition metals better conductors than alkali metals?
transition metals
Is a cation isoelectric with the element before or after it?
No necessarily. Although the alkali metal cations are, most other cation-forming elements (metals) are not as many of them lose more than one electron. It is even more complicate for the transition metals as they can move electrons between their s and d orbitals.
Transition metals most often form ions with what charge?
most transition metals form ions with a 2+ charge.
What metals have electrons added to their d-orbitals and often do not exhibit regular or predictive electron configurations?
The transition metals
What metals have electrons added to their d orbitals and often do not exhibit regular or predictive electron configuration?
The transition metals
Why are alkali metals more reactive than transition metals?
Groups 3-12 do not have individual names. Instead, all of these groups are called transition metals. The atoms of transition metals do not give away their electrons as easily as atoms of the Group 1 and Group 2 metals do. So, transition metals are less reactive than alkali metals and alkaline-earth metals are.
How does the electron configuration contributes to transition metals?
color, magnetism, conductivity to name a few.
Why are the properties of the elements in a group are usually similar?
Take the alkali earth metals as an example, column I in the Periodic Table. All of them have an unpaired s electron in their outer shell. All of them will form a +1 cation. When you go down the column, all of them will have a similar outer shell configuration. The transition metals are different, however.
A colored ion generally indicates a?
The presence of a transition metal.Read more: A_colored_ion_generally_indicates_what
How does the arrangement of alkali earth metals make them very reactive?
Alkalis have one electron in their valency shells. They can "lose" this electron easily, forming a cation which is strongly reactive.
Is cations the same thing as covalent bonds?
No. A cation is the element becoming ion that donates an electron to an ionic bond( generally metals ). Covalent bonds are shared electron bonds.
Why do transition metals share properties with other transition metals in their period?
The physical properties of transition metals are determined by their electron configurations. Most transition metals are hard solids with relatively high melting and boiling points. Differences in properties among transition metals are based on the ability of unpaired d electrons to move into the valence level. The more unpaired electrons in the d sublevel, the greater the hardness and the higher the melting and boiling points.
Why do metals share properties with other transition metals in their period?
The physical properties of transition metals are determined by their electron configurations. Most transition metals are hard solids with relatively high melting and boiling points. Differences in properties among transition metals are based on the ability of unpaired d electrons to move into the valence level. The more unpaired electrons in the d sublevel, the greater the hardness and the higher the melting and boiling points.
