Identify the outer electron configurations for the (a) alkali metals, (b) alkaline earth metals, (c) halogens, (d) noble gases.

 

For each electronic configuration given, choose the electronic configuration of the element that would match its chemical properties. 

(a) 

 

(b) 

  

(c) 

   

Group the following electron configurations in pairs that would represent elements with similar chemical properties. only check there boxes. 

  

Without referring to a periodic table, write the electron configuration of the elements with the following atomic numbers.
(a) Z = 9:
(b) Z 20:
(c) Z - 26:
(d) Z - 33:
A M ²⁺ ion has four electrons in the 3d subshell and is derived from a metal in the first transition metal series. What element might M be?
Elemental symbol: _____

Write ground—state electron configurations for these ions, which play important roles in biochemical processes in our bodies. (Use a noble gas core abbreviation.)
(a) Na ⁺ ___
(b) mg ²⁺ ___
(c) CI ^- ___

(d) K ⁺ ___

Within each group of four atoms or ions presented below, select the species that are isoelectronic with each other:

Zn ………………………….Ge ²⁺

Fe ³⁺ ……………………….CI ^-

Mn ²⁺ ………………………B ^-

Ar -----------------------C

Drag each item to the correct box.

Arrange the following atoms in order of decreasing atomic radius:

A) Cs

B) K

C) Mg

D) Al

E) Na

F) CI

G) P 

   

Classify the following bonds as covalent, polar covalent, or ionic.

(a) The bond in CsCI

Covalent

Polar

Covalent ionic

(b) The bonds in H ₂ S

Covalent polar covalent ionic

 

(c) The NN bond in II H₂ NNH₂  

 

Covalent

Polar

Covalent ionic 

Draw the Lewis structure of sulfur tetrafluoride (SF₄).  

(a) Alkali metal (b) Alkaline earth (c) Halogens (d) Noble gases metals A. ns' A. ns! A. ns' A. ns! . ns 2 . ns 2 . ns 2 B. ns C. ns np' C. ns np' C. ns np' . ns? 2 2 D. ns np D. ns np" D. ns np? D. ns np E. ns np E. ns E. ns E. ns F. ns np* F. ns np" F. ns np O F. ns np4 G. ns np G. ns np3 G. ns? np5 O G. ns np5 6. H. ns np H. ns np H. ns np . ns * 2.