Pls why the metal activity of the zinc group is higher than that of the copper group

Pure zinc is more stable than copper and not with hydrochloric acid. What we usually see is zinc with impurities.

zn: Because the electronic structure is [ar], d and s are fully filled, it is not easy to lose electrons. So the i1 is bigger.

It can be seen that the ionization energy of Zn is greater than that of Cu, and in fact, Zn is more reactive than Cu, proving that the reactivity cannot be judged by ionization energy alone. In fact, it is necessary to comprehensively consider the two aspects of gaining and losing electronic capabilities.

In terms of the general trend, the ionization energy of the long period increases with the increase of z, but there is an anomaly. The decrease in the radius of the subgroup elements is small, that is, the increase in z* is small, and the gravitational increase in the outer electrons is small, so the increase in i is also small. Sometimes there are anomalies.

Electronegativity calculation:

In 1934, Millikan proposed: x = 1 2(i + e) (electronegativity is half of the sum of ionization energy and electron affinity energy) In this way, the absolute electronegativity value can be calculated. However, due to the lack of data on e, this formula has limitations in its application.

In 1957, Allred-Rochow, introducing the effective nuclear charge z*, proposed that the gravitational force of the check electron is:

two constants are introduced; The results of the calculations are in good agreement with the Pauling data.

Electronegativity comparison: xcu = , zn = , so cu is less likely to lose electrons than zn, i.e., cu is more metallic. This is a combination of ionization energy and electron affinity energy.

The peripheral electron configuration of copper is 3d104s1, which is semi-filled, the shielding effect is small, and the gravitational attraction of the outer electrons is large.

There is such an explanation: on the outermost shell, copper has only one electron, while zinc has two electrons with opposite spin directions, which have a large repulsive force and are easy to lose, so its metallicity is stronger.

Note that copper is d10s1, not d9s2.

To put it simply, copper is semi-filled and relatively stable (this theory seems to be something that cannot be proven), and it is not clear what electronegativity and orbital radius are when it comes to it, as long as you know. After all, chemistry is different from physics, and there are too many theories that have "exceptions" for various reasons.

The metallicity of copper and zinc cannot be derived from the periodic law, and the periodic law studied in high school is for the main group of elements. It is certain that the metallicity of copper is weaker than that of zinc, and there is no need to be entangled in the paragroup elements in high school learning, and it is enough to recite the metallicity of common elements.

No, the metallicity of Zn is much greater than that of Cu. As said on the first floor, it is metal sex table on it. Furthermore, the valence electron configuration of Cu is 3d9 4s1 and Zn's is 3d10 4s2.

Comparatively, Zn has a greater first ionization energy than Cu, that is, the harder it is to lose the first electron, the weaker the oxidation, and the stronger the reduction. (That general conclusion should be mainly applied to the main element.)

Electronegativity (Cu)= (Zn)= . Electronegativity can exhibit the electrophilicity of an element, and the greater the electronegativity, the stronger the electrophilicity. The electronegativity of Zn is smaller than that of Cu, and the electrophilicity is smaller, so it is easy to lose electrons.

The properties of the main group elements and the short-term and medium-term elements cannot be recursively inferred to the minor group elements, and the periodic law properties you are talking about only apply to the main group elements and the short-term and medium-term elements. It is said in the university "Inorganic Chemistry".

i(Cu) = i(Zn) = Zn is greater than the first ionization energy of Cu, the harder it is to lose the first electron, the weaker the oxidation, and the stronger the reduction.

No, copper is less metallic than zinc.