"Positive" and "negative" are just terms that we assign to define a fundamental difference in the way charges interact. We could just as well call them "up" and "down", or "blue" and "red" - the words you chose don't affect the physics.
The point is that they are different and that difference is what causes the unique interactions we observe.
Zinc is the anode.
It depends on the specifics of the cell, but in most simple galvanic cells, the anode slowly dissolves into solution.
A galvanic cell is a spontaneous reaction so electron flow will occur as long as a salt bridge is present.
The Anode in electrochemical cell has negative charge (-ve).
Electrons flow in the opposite direction.
Zinc is the anode.
The electrode that is oxidized in a galvanic cell ~
The electrode with the highest oxidation potential
It can be complicated depending on the type of cell one is looking at. However, here is my simple explanation.The anode is the electrode where the oxidation reaction takes place, and oxidation is the loss of electrons, so in a galvanic cell the anode is a source of free electrons and so it is negatively charged.The cathode is the electrode where reduction takes place, and reduction is the gain of electrons, so in a galvanic cell the cathode is positively charge and ready to accept negatively charged electrons.Now, the anode isn't always negative and the cathode isn't always positive. It has to do with the direction of current flow (anode = current in, cathode = current out). In an electrolytic cell, the charges on the anode and the cathode are reversed from that seen in a galvanic cell.
It depends on the specifics of the cell, but in most simple galvanic cells, the anode slowly dissolves into solution.
A galvanic cell is a spontaneous reaction so electron flow will occur as long as a salt bridge is present.
The Anode in electrochemical cell has negative charge (-ve).
Electrons flow in the opposite direction.
This is the anode.
The Cathode is the negative electrode; the anode is the positive electrode
Two electrodes in electrolyte solutions
The electrolyte of a commercial galvanic cell normally extends from anode to cathode without interruption by a salt bridge. A salt bridge is normally a teaching tool to help show that: 1. Galvanic half-cells do not produce voltage 2. Conductors and insulators are not necessarily salt bridges. An electrolyte must extend from anode to cathode before the galvanic cell can produce voltage. 3. The chemical composition of the salt bridge can differ from the electrolytes in the half cells. 4. Ions travel through the salt bridge between the cell's anode and cathode. Salt bridges raise more questions than answers. For example: 1. Can the difference between an electrolyte and a conductor be defined? 2. How do ions quickly move through a solid or a long electrolyte? 3. When salt bridge composition differs from the galvanic cell electrolyte(s), must the salt bridge chemically react with the galvanic cell electrolyte(s)? 4. Why does galvanic cell voltage remain nearly constant while anode to cathode distance doubles.